Quiz 15: How Atoms Bond and Molecules Attract
Physics & Astronomy
Q 1Q 1
What is the valence shell?
A)It is the outermost shell of electrons in an atom.
B)It is the shell of electrons in an atom that is the least reactive.
C)It is the last partially filled orbital in an atom.
D)It is the shell of electrons in element V (atomic no.= 23)
E)It is the same as the orbital configuration.
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A
Q 2Q 2
The concept of a chemical bond is
A)how two or more atoms are held together.
B)the sharing of nucleons.
C)how two or more electrons reside in an orbital.
D)how much energy it takes to remove an electron from a set of atoms.
E)none of the above
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A
Q 3Q 3
Many of the macroscopic properties of a compound depend on
A)how the atoms of the molecules are held together.
B)the mass of the constituent atoms.
C)the number of nucleons present in the sample.
D)the size of the sample.
E)how the atoms absorb light and the shape of the orbitals.
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A
Q 4Q 4
Which of the following is the correct electron dot structure for chlorine (atomic no.= 17)?
A)a
B)b
C)c
D)d
E)e
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Q 5Q 5
Which of the following is the correct electron dot structure for carbon (atomic no.= 6)?
A)a
B)b
C)c
D)d
E)e
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Q 6Q 6
Which of the following has the greatest number of nonbonding pairs of electrons?
A)C
B)H
C)He
D)F
E)S
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Q 12Q 12
What is one role of unpaired valance electrons?
A)They take part in the formation of different types of bonds.
B)They keep the paired electrons separated to minimize interaction.
C)They are the nonbonding electrons.
D)They provide the number of Lewis dots.
E)They tell us which Lewis dot structure is correct.
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Q 13Q 13
How do the electron-dot structures of elements in the same group in the periodic table compare with one another?
A)The structures differ by exactly two electrons between vertically consecutive elements.
B)The number of valence shell electrons increases by one for each element from the top to the bottom of the group.
C)Elements of the same group have the same number of valence electrons.
D)The number of electrons in the electron-dot-structure will equal the group number for each element of the group.
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Q 14Q 14
How many more electrons can fit within the valence shell of a hydrogen atom?
A)1
B)2
C)7
D)0
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Q 15Q 15
How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form?
A)There is no defined relationship between the number of unpaired valence electrons and number of bonds that the atom can form.
B)The number of unpaired valence electrons in an atom is one-half the number of bonds that the atom can form.
C)The number of unpaired valence electrons in an atom is twice the number of bonds that the atom can form.
D)The number of unpaired valence electrons in an atom is the same as the number of bonds that the atom can form.
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Q 16Q 16
Why is it so easy for a magnesium atom to lose two electrons?
A)The nuclear charge of the magnesium atoms is relatively weak.
B)These two electrons are found relatively far from the nucleus.
C)These two electrons are well shielded from the nuclear charge.
D)There are lots of electron-electron repulsions that go on within the valence shell.
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Q 17Q 17
An atom loses an electron to another atom.Is this an example of a physical or chemical change?
A)physical change involving the formation of negative ions
B)chemical change involving the formation of neutral atoms
C)physical change involving the formation of positive ions
D)chemical change involving the formation of ions
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Q 18Q 18
How is it possible for a neutral molecule,such as water,to form an ion?
A)It can combine with a hydrogen ion to form a positively charged species.
B)It can combine with a chloride ion to form a negatively charged species.
C)It can fragment into protons and electrons.
D)It can absorb electrons and become negatively charged.
E)It can absorb electrons and become positively charged.
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Q 19Q 19
If carbonic acid (H2CO3)were to undergo ionization,what would one of the products be?
A)H-
B)CO2
C)H2O
D)CO3-1
E)CO3-2
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Q 20Q 20
What is the name for the following polyatomic ion? CH3CO2-1
A)acetate
B)monocarboxylate
C)carboxylic
D)acidic
E)acetic
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Q 21Q 21
What is the name for the following polyatomic ion? PO4-3
A)phosphate
B)phosphorus oxide
C)phosphinate
D)trioxo phosphoride
E)potassium
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Q 22Q 22
Which of the following elements will most likely not form an ion at all?
A)Na
B)O
C)Ar
D)Mg
E)Br
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Q 23Q 23
Which of the following elements will most likely form an ion with a -1 charge?
A)Na
B)S
C)Ne
D)Mg
E)Cl
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Q 24Q 24
Which of the following elements will most likely form an ion with a -2 charge?
A)Na
B)S
C)Ne
D)Mg
E)Cl
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Q 25Q 25
Which of the following elements will most likely form an ion with a +2 charge?
A)Na
B)Mg
C)Ne
D)Si
E)Cl
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Q 26Q 26
Which of the following elements will most likely form an ion with a +1 charge?
A)Na
B)Mg
C)Al
D)Si
E)Cl
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Q 27Q 27
Which of the following would be an ion with a double positive charge?
A)an Mg atom that gains two electrons
B)an Mg atom that gains one electron
C)an Mg atom that loses two electrons
D)an Mg atom that loses one electron
E)none of the above
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Q 28Q 28
Which of the following would be a negative ion with a single charge?
A)an atom with 11 protons and 12 electrons
B)an atom with 11 protons and 11 electrons
C)an atom with 12 protons and 11 electrons
D)an atom with 10 protons and 12 electrons
E)none of the above
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Q 31Q 31
What needs to be done to convert a neutral nitrogen atom into an N-3 species?
A)add three electrons
B)remove three electrons
C)remove three protons
D)add three protons
E)add three nitrogens
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Q 32Q 32
If a neutral atom gains two electrons,what is the electrical charge of the atom?
A)-1
B)+1
C)-2
D)+2
E)neutral
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Q 33Q 33
If a neutral atom loses one electron,what is the electrical charge of the atom?
A)-1
B)+1
C)-2
D)+2
E)neutral
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Q 36Q 36
The neon atom tends not to lose any electrons because
A)of its relatively strong effective nuclear charge.
B)that would result in a negative ion.
C)its electrons are paired together within the same orbitals.
D)the ionization energy is so high.
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Q 37Q 37
The neon atom tends not to gain any additional electrons because
A)its nuclear charge is not great enough.
B)that would result in a positive ion.
C)of the repulsions they would experience with electrons in the same shell.
D)there is no more room available in its outermost occupied shell.
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Q 38Q 38
Why doesn't the sodium atom gain seven electrons so that its third shell becomes the filled outermost shell?
A)It would be too difficult for another atom to lose seven electrons.
B)Only six additional electrons are required to fill the outermost shell of sodium.
C)In gaining seven more electrons,sodium's fourth outer shell becomes filled.
D)Sodium's nuclear charge is not strong enough to hold that many more electrons.
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Q 39Q 39
Which should be larger,the potassium atom,K,or the potassium ion,K⁺?
A)The potassium ion,K⁺ is larger since charging an atom always makes it larger.
B)The potassium atom,K,with an additional shell of electrons is larger.
C)The potassium ion,K⁺ is larger since it has an extra electron which increases its size.
D)The potassium atom and the potassium ion are exactly the same size and only differ in charge.
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Q 40Q 40
Why does an atom with many valence electrons tend to gain electrons rather than lose any?
A)Atoms with many valence electrons tend to have relatively weak forces of attraction between the valence electrons and the nucleus.Therefore,the outer electrons are free to attract other electrons.
B)There is stability in numbers.Atoms with many valence electrons are always attracting new electrons.
C)The old adage that "he who has,gets" is also true in atomic structure.Atoms with many valence electrons can essentially overpower atoms with few valence electrons and attract additional electrons.
D)Atoms with many valence electrons tend to have relatively strong forces of attraction between the valence electrons and the nucleus.This makes it easy for them to gain additional electrons.
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Q 41Q 41
Take money away from your bank account and the bank will show a negative credit.Take an electron away from an atom,however,and the atom shows up positive.Explain.
A)Electrons are already negative.Therefore,we know from basic math that subtracting a negative (number)from a neutral (atom),will make the result positive.
B)Neutral atoms contain identically charged but oppositely signed protons and electrons.Removing one of the negative electrons results in an excess of positively charged protons.
C)Removing an electron from an atom does not have the atom show up positive.It simply leaves the atom short one electron.
D)Atoms are constantly exchanging electrons.Having an atom "show up positive" is only an expression indicating that it has taken its turn in the game of electron exchange.
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Q 42Q 42
Which of the following best describes ionic bonding?
A)two atoms sharing a set of electrons
B)two atoms exchanging a set of electrons
C)one atom giving up some of its electrons to another atom
D)when two elements with same charge are held together by electrostatic forces
E)none of the above
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Q 43Q 43
Which of the following molecules contains an ionic bond?
A)MgCl2
B)Cl2
C)SF3
D)PO4-3
E)none of the above
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Q 44Q 44
If the following generic atom were to undergo ionization,what would the most likely product be?
A)+1
B)-2
C)-3
D)+4
E)would probably not ionize
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Q 45Q 45
If the following generic atom were to undergo ionization,what would be the charge of the most likely product?
A)+2
B)-2
C)-6
D)+6
E)would probably not ionize
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Q 46Q 46
If the following generic atom were to undergo ionization,what would be the charge of most likely product?
A)+3
B)-3
C)-5
D)8
E)would probably not ionize
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Q 47Q 47
What is the compound that forms if you react potassium and sulfur?
A)K2S
B)KS
C)SP
D)PS2
E)SkP
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Q 48Q 48
If you mix a typical aluminum ion (Al,atomic no.= 13)with a typical oxygen ion (O,atomic no.= 8),what compound is formed?
A)Al2O3
B)Al3O2
C)Al13O8
D)Al3O
E)Al2O2
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Q 49Q 49
If you mix a typical iodine ion (I,atomic no.= 53)with a typical barium ion (Ba,atomic no.= 56),what compound is formed?
A)BaI2
B)BaI
C)Ba56I53
D)Ba2I
E)Ba2I2
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Q 50Q 50
How many oxide ions (O-2)are needed to balance the positive charge of a titanium ion (Ti+4)?
A)2
B)1
C)3
D)4
E)6
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Q 51Q 51
How many chloride ions (Cl-1)are needed to balance the positive charge of a barium ion (Ba+2)?
A)2
B)1
C)-2
D)-1
E)3
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Q 52Q 52
Which are closer together: the two nuclei within potassium fluoride,KF,or the two nuclei within molecular fluorine, ?
A)KF
B)
C)Both are the same.Any atom bonded to F will have the same inter-nuclear separation.
D)It makes little sense to compare two molecules which exist in different physical states.KF is a solid while
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Q 53Q 53
Which would you expect to have a higher melting point: sodium chloride,NaCl,or aluminum oxide, ?
A)The aluminum oxide has a higher melting point because it is a larger molecule and has a greater number of molecular interactions.
B)NaCl has a higher melting point because it is a solid at room temperature.
C)The aluminum oxide has a higher melting point because of the greater charges of the ions,and hence the greater force of attractions between them.
D)The aluminum oxide has a higher melting point because of the covalent bonds within the molecule.
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Q 54Q 54
Is an ionic compound an example of a chemical compound,or is a chemical compound an example of an ionic compound?
A)An chemical compound is an example of a ionic compound.
B)Neither is an example of the other.
C)Each is an example of the other.
D)An ionic compound is an example of a chemical compound.
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Q 55Q 55
What molecule loses a proton to form the hydroxide ion,OH⁻?
A)the oxygen molecule,
B)the water molecule, O
C)the hydrogen peroxide molecule,
D)the hydrogen molecule,
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Q 56Q 56
Barium ions carry a 2+ charge,and nitrogen ions carry a 3- charge.What would be the chemical formula for the ionic compound barium nitride?
A)
B)
C)
D)
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Q 57Q 57
Magnesium ions carry a 2+ charge,and chloride ions carry a 1- charge.What is the chemical formula for the ionic compound magnesium chloride?
A)MgCl
B) Cl
C)Mg
D)
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Q 60Q 60
Which of the following does not describe ionic compounds?
A)They have a tendency to melt easily.
B)They consist of positive and negative ions.
C)They are held together by electrostatic attraction.
D)They are usually very ordered.
E)none of the above
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Q 61Q 61
Which would you expect to have a higher melting point: sodium chloride,NaCl,or cesium chloride,CsCl? Why?
A)The cesium chloride has a higher melting point because larger ions of the same charge are able to attract more ions of the opposite charge.
B)The cesium chloride has a higher melting point because its ions are smaller,which makes the charges more dense.
C)The sodium chloride has a higher melting point because of the greater charges of the ions,and hence the greater force of attractions between them.
D)The sodium chloride has a higher melting point because its ions are smaller,which allows oppositely charged ions to get closer.
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Q 62Q 62
crystals are composed of
A)units of molecules held together by dipole interactions.
B)groups of ions and molecules.
C)units composed of six Mg atoms and six molecules.
D)a multitude of ions and ions grouped together in a three-dimensional array with a 1:2 ratio of to .
E)a two-dimensional array of [-Mg-Cl-Cl-] units.
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Q 63Q 63
Which of the following is not a property of metal?
A)does not conduct heat well
B)conducts electricity
C)is shiny
D)is strong,but can be bent
E)All of the above are properties of metals.
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Q 64Q 64
Metals are useful for the structural support of buildings because they
A)do not conduct heat well.
B)are shiny.
C)conduct electricity.
D)are strong but can be bent.
E)c and d
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Q 65Q 65
Metals are often used for making designer jewelry because they
A)do not conduct heat well.
B)conduct electricity.
C)are shiny.
D)are strong but can be bent.
E)c and d
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Q 66Q 66
What property of metal atoms account for many of the observed bulk phenomena seen in metal samples?
A)Metal atoms easily lose one or more outer electrons.
B)Metal atoms easily gain one or more outer electrons.
C)Metals readily form ionic bonds.
D)Metals readily form covalent bonds.
E)none of the above
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Q 67Q 67
Which of the following describes how a metal atoms behaves in a bulk metallic object?
A)The metal ion shares its outermost electrons freely with its neighbors.
B)The metal atoms have limited interaction with neighboring atoms.
C)The metal atom shares its electrons in a very directional manner.
D)The metal atom shares its electrons with only one other atom.
E)none of the above
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Q 68Q 68
Given that the total number of atoms on our planet remains fairly constant,how is it ever possible to deplete a natural resource such as a metal?
A)The problem remains that not everyone recycles as they should.
B)Recycling only forestalls the inevitable depletion of metal resources.
C)The atoms don't leave our planet,which is why naturally occurring materials never really reach the point of depletion.
D)The problem is with the expense of collecting metal atoms that are uniformly dispersed.
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Q 69Q 69
Distinguish between a metal and a metal-containing compound.
A)There is no distinction between the two.
B)Only one of these contains ionic bonds.
C)Only one of these contains covalent bonds.
D)Only one of these occurs naturally.
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Q 70Q 70
Why are ores so valuable?
A)They are sources of naturally occurring gold.
B)Metals can be efficiently extracted from them.
C)They tend to occur in scenic mountainous regions.
D)They hold many clues to Earth's natural history.
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Q 71Q 71
Why is it better to recycle metals than to mine more?
A)It takes far less energy to recycle.
B)Mining is less expensive than recycling but not environmentally friendly.
C)Ores contain toxic elements.
D)all of the above
E)none of the above
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Q 72Q 72
There is more gold in 1 km3 of the ocean than the amount of gold mined in all of recorded history.How come we do not mine the oceans?
A)It is too dilute to separate.
B)It would take too much energy.
C)It would cost too much.
D)all of the above
E)none of the above
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Q 73Q 73
If the concentration of gold in seawater is 2.0 milligram per ton of sea water and the mass of the ocean is 1.5 × 1018 tons,how much gold is in the ocean?
A)3.0 × 1012 kg
B)3.0 kg
C)300 g
D)36 mg
E)3000 lb
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Q 74Q 74
What property of alloys make them ideal for developing new materials?
A)The characteristics of the material change depending on how much of each component is present.
B)Alloys are very rigid and are extremely resistant to chemical decomposition.
C)The size of the atoms involved is directly related the electrical conductivity.
D)all of the above
E)none of the above
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Q 75Q 75
Why is metal shiny?
A)The loose electrons reflect most wavelengths of light.
B)The electrons transmit most wavelengths of light.
C)The electrons absorb each light wave.
D)The electrons emit light due to electronic excitation.
E)all of the above
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Q 76Q 76
What is a molecule?
A)a group of atoms that are held together by covalent bonds
B)a group of atoms that are held together by ionic bonds
C)pair of atoms sharing a set of valence electrons
D)pair of shared valence electrons
E)group of covalent compounds held together by ionic bonds
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Q 77Q 77
What it the main difference between an ionic and a covalent bond?
A)One is the sharing of a pair of electrons,the other is the transfer of at least one electron.
B)One involves electrons,the other does not involve any electrons.
C)The electrons in both types of bonding undergo an exchange.
D)The electrons are traded between the two atoms and this keeps the atoms close.
E)Both bonds are the same,but named different to describe different atoms involved.
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Q 78Q 78
What does the line in the following example actually represent? H-H
A)a shared pair of electrons
B)a covalent bond
C)an ionic bond
D)a pair of nonbonding electrons
E)A and B
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Q 79Q 79
How many nonbonding pairs of electrons are in the following molecule? H-H
A)1 pair
B)6 pairs
C)0 pairs
D)8 pairs
E)none of the above
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Q 80Q 80
How many covalent bonds would the following atom usually form?
A)1
B)2
C)4
D)6
E)It would tend to form ionic bonds.
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Q 81Q 81
How many covalent bonds would the following generic atom usually form?
A)1
B)2
C)4
D)8
E)would usually not form any covalent bonds
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Q 82Q 82
How many covalent bonds would the following atom usually form?
A)3
B)2
C)1
D)5
E)would usually not form any covalent bonds
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Q 83Q 83
Which of the following statements is untrue?
A)Covalent molecules are never crystalline.
B)Covalent molecules usually have low melting points.
C)Covalent molecules can have nonbonding electrons.
D)Covalent bonds can involve more than one pair of electrons.
E)All of the above statements are true.
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Q 84Q 84
Classify the following bonds as ionic,covalent,or neither (O,atomic number 8; F,atomic number 9; Na,atomic number 11; Cl,atomic number 17; U,atomic number 92). O with F Ca with Cl Na with Na
A)covalent,ionic,covalent
B)ionic,covalent,neither
C)neither,ionic,covalent
D)covalent,ionic,neither
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Q 85Q 85
Which of the following substances is pure?
A)an ionic compound consisting of sodium and chlorine ions
B)a covalent compound consisting of one type of molecule
C)an element
D)all of the above
E)none of the above
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Q 86Q 86
Which of the following statements best describes a relatively polar bond?
A)a very electronegative atom and a weakly electronegative atom are covalently bound
B)two very electronegative atoms are covalently bound
C)two very electronegative atoms undergo ionic bonding
D)two weakly electronegative atoms undergo ionic bonding
E)none of the above
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Q 87Q 87
Which of the following molecules would contain a dipole?
A)H-F
B)Cl-Cl
C)H-H
D)F-F
E)all of the above
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Q 88Q 88
Which of the following molecules contains a polar bond?
A)H-F
B)Cl-Cl
C)H-H
D)F-F
E)all of the above
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Q 89Q 89
Which of the following bonds would be the most polar?
A)C-F
B)C-Cl
C)C-Br
D)C-I
E)All are equally polar.
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Q 90Q 90
Which of the following bonds would be the least polar?
A)C-F
B)C-O
C)C-Cl
D)C-H
E)All are equally polar.
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Q 92Q 92
Does an ionic bond have a dipole?
A)No,dipoles are only found in covalent compounds.
B)No,but the electrical charges are relatively strong.
C)Yes,the ionic bond is an example of a very strong dipole.
D)Yes,but for ionic compounds they are referred to as monopoles.
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Q 93Q 93
The source of an atom's electronegativity is the
A)repulsive force occurring among electrons within the same shell.
B)repulsive force occurring between electrons within neighboring shells.
C)positively charged atomic nucleus.
D)kinetic energy electrons have orbiting the nucleus.
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Q 94Q 94
In terms of the periodic table,is there an abrupt or gradual change between ionic and covalent bonds?
A)There is an abrupt change that occurs across the metalloids.
B)Actually,any element of the periodic table can form a covalent bond.
C)There is a gradual change: the farther apart,the more ionic.
D)Whether an element forms one or the other depends on nuclear charge and not the relative positions in the periodic table.
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Q 95Q 95
Atoms of nonmetallic elements form covalent bonds,but they can also form ionic bonds.How is this possible?
A)This happens when one of the bonded nonmetallic elements has a strong electronegativity.
B)It happens when one of the nonmetallic elements loses an electron to become a positive ion.
C)An ionic bond results when a nonmetallic elements loses an electron to a metallic element.
D)An ionic bond results when a nonmetallic elements gains an electron from a metallic element.
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Q 96Q 96
Atoms of metallic elements can form ionic bonds,but they are not very good at forming covalent bonds.Why?
A)These atoms are too large to be able to come in close contact with other atoms.
B)They have a great tendency to lose electrons.
C)Their valence shells are already filled with electrons.
D)They are on the wrong side of the periodic table.
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Q 98Q 98
Which is more polar,a sulfur-bromine (S-Br)bond or a selenium-chlorine (Se-Cl)bond?
A)A selenium-chlorine bond should be more polar because of a greater difference in effective nuclear charge.
B)A selenium-chlorine bond should be more polar because of a smaller difference in effective nuclear charge.
C)A sulfur-bromine bond should be more polar because of a greater difference in effective nuclear charge.
D)A sulfur-bromine bond should be more polar because of a smaller difference in effective nuclear charge.
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Q 99Q 99
-Which of the following molecules is polar?
A)a
B)b
C)c
D)All are polar.
E)Only A and C are polar.
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Q 100Q 100
-Which of the above substances would have the lowest boiling point?
A)a
B)b
C)c
D)All boil at the same temperature.
E)All are gases.
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Q 101Q 101
-Which of the above substances would have the largest dipole?
A)a
B)b
C)c
D)Each has the same size dipole.
E)None of the molecules has a dipole.
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Q 102Q 102
-Which of the following molecules has the highest boiling point?
A)BH3
B)NH3
C)CH4
D)All of the above should have the same boiling point.
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Q 103Q 103
-Which of the following statements describes a polar molecule?
A)The electrons in the molecule are distributed evenly throughout the molecule.
B)The molecules are usually not attracted to one another very strongly.
C)Polar molecules have the weakest intermolecular interactions with ionic compounds.
D)The molecules have a high degree of symmetry.
E)None of these statements describe polar molecules.
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Q 104Q 104
-Which of the following molecules should have the same molecular shape and approximate bond angles as ammonia, ?
A)
B)
C)
D)
E)
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Q 107Q 107
List the following bonds in order of increasing polarity.
A)N-O < N-N < N-F < H-F
B)N-N < N-O < N-F < H-F
C)H-F < N-F < N-O < N-N
D)N-N < N-O < H-F < N-F
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Q 108Q 108
Water, O,and methane,C ,have about the same mass and differ by only one type of atom.Why is the boiling point of water so much higher than that of methane?
A)The water molecule is less symmetrical than is the methane molecule.
B)The oxygen of a water molecule has two lone pairs of electrons.
C)The electronegativity difference between oxygen and hydrogen is greater than the electronegativity difference between carbon and hydrogen.
D)all of the above
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Q 109Q 109
An individual carbon-oxygen bond is polar.Yet carbon dioxide,C ,which has two carbon-oxygen bonds,is nonpolar because
A)the molecule has an even number of electrons.
B)it has a greater symmetry.
C)the electron-pulls of the two oxygen atoms are equal and opposite.
D)Two of the above are reasonable.
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Q 110Q 110
A substance consisting of which molecule shown below should have a higher boiling point?
A)The molecule on the left,CO ,because it has a fewer number of atoms.
B)The molecule on the right, Cl,because it has a greater number of atoms.
C)The molecule on the left,CO ,because it is less symmetrical.
D)The molecule on the right,
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Multiple Choice
Q 111Q 111
Ammonia,N ,is more polar than is borane,B because it
A)has a lone pair of electrons.
B)is less symmetrical than borane.
C)its hydrogens are not exactly opposite one another.
D)all of the above
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Multiple Choice
Q 112Q 112
Which of the following is the weakest?
A)a chemical bond
B)an ion-dipole attraction
C)a dipole-dipole attraction
D)a dipole-induced dipole attraction
E)an induced dipole-induced dipole attraction
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Multiple Choice
Q 113Q 113
Which of the following is the strongest?
A)a chemical bond
B)an ion-dipole attraction
C)a dipole-dipole attraction
D)a dipole-induced dipole attraction
E)an induced dipole-induced dipole attraction
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Multiple Choice
Q 114Q 114
Which of the following molecules would you expect to be the least attracted to a Na+ ion?
A)H-F
B)H3C-CH3
C)Cl2CH2
D)F-
E)HO-
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Multiple Choice
Q 115Q 115
Which of the following molecules would you expect to be the most strongly attracted to a Cl- ion?
A)H-F
B)H3C-CH3
C)Cl-Cl
D)F-F
E)CCl4
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Multiple Choice
Q 116Q 116
The separation of charges within a polar molecule is called a(n)
A)dipole.
B)dipole-dipole.
C)ionic bond.
D)strong attraction.
E)polar bond.
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Multiple Choice
Q 117Q 117
What is happening at the molecular level when a polar molecule like water interacts with a typical sodium ion?
A)The water molecule aligns such that the oxygen interacts with the sodium.
B)The water molecule aligns such that the hydrogens interact with the sodium.
C)The polarity of the water molecule is altered making the oxygen more positively charged.
D)The polarity of the water molecule is altered making the hydrogens more negatively charged.
E)none of the above
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Multiple Choice
Q 118Q 118
If an ionic bond is stronger than a dipole-dipole interaction,how can water dissolve an ionic compound?
A)The ion-dipole interactions of a bunch of water molecules gang up on the strong ionic bond and pull it into the solution.
B)The ionic bond is weakened by the ion-dipole interactions and ionic repulsion ejects the ions from the crystal.
C)The ion-dipole interaction causes the ions to heat up and vibrate free of the crystal.
D)The ions never overcome their interatomic attraction and therefore are not soluble.
E)none of the above
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Multiple Choice
Q 119Q 119
What is the difference between a dipole-dipole interaction and an ion-dipole interaction?
A)one involves dipole attraction between neutral molecules while the other involves dipole interactions with ions
B)one involves hydrogen bonding while the other does not
C)one involves salts and water while the other doesn't involve water
D)one involves ionic molecules interacting with other ionic molecules while the other deals with polar molecules
E)none of the above
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Multiple Choice
Q 120Q 120
Which of the following describes an aqueous solution?
A)a mixture of some compound dissolved in water
B)a mixture of polar molecules dissolved in a nonpolar solvent
C)a mixture of water dispersed in an ionic compound
D)a mixture of nonpolar molecules dissolved in a polar solvent
E)none of the above
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Multiple Choice
Q 121Q 121
What is a hydrogen bond?
A)a special type of dipole-dipole attraction involving hydrogen bound to a highly electronegative atom
B)a special type of dipole-dipole attraction involving hydrogen bound to any other atom
C)a special type of dipole-dipole attraction involving hydrogen bound to another hydrogen atom
D)a special type of attraction involving any molecules that contain hydrogens
E)none of the above
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Multiple Choice
Q 122Q 122
Which of the following molecules is most likely to show the strongest hydrogen bonding?
A)CH3OH
B)CH3SH
C)CH4
D)H-C C-H
E)A,B and C
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Multiple Choice
Q 123Q 123
Which of the following molecules is most likely to show a dipole-dipole interaction?
A)CH3OH
B)CH3SH
C)CH4
D)H-C C-H
E)A and B
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Multiple Choice
Q 124Q 124
Which of the following molecules is most likely to show a dipole-dipole interaction?
A)H2S
B)CO2
C)CH4
D)H-C C-H
E)none of the above
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Multiple Choice
Q 125Q 125
Which of the following is the main form of intermolecular attractions among water molecules?
A)hydrogen bonding
B)induced dipole-induced dipole
C)covalent bonding
D)ion-dipole
E)polar-induced polar
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Multiple Choice
Q 126Q 126
Given the following diagram,describe what happens electronically between these two molecules.
A)Oxygen B becomes slightly positively charged due to the electrons on the water molecule.
B)Oxygen A becomes slightly positively charged due to the electrons on the water molecule.
C)Oxygen W becomes slightly negatively charged due to the oxygen molecule.
D)Oxygen W becomes slightly positively charged due to the oxygen molecule.
E)none of the above
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Multiple Choice
Q 127Q 127
Given the following diagram,describe what happens electronically between these two molecules.
A)Oxygen A becomes slightly positively charged due to the protons on the water molecule.
B)Oxygen B becomes slightly positively charged due to the protons on the water molecule.
C)Oxygen A becomes slightly negatively charged due to the oxygen molecule.
D)Hydrogens on oxygen W becomes slightly positively charged due to the oxygen molecule.
E)none of the above
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Multiple Choice
Q 128Q 128
In which of the following molecules will water induce a temporary dipole?
A)CO2
B)O2
C)N2
D)all of the above
E)none of the above
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Multiple Choice
Q 129Q 129
What is the main difference between a dipole-dipole interaction and a dipole-induced dipole interaction?
A)Both are similar,but one involves a temporary dipole created by a permanent dipole.
B)Dipole-dipole interactions are weaker because the dipoles are permanent.
C)Dipole-induced dipole interactions are stronger because the induced dipoles can be formed at any time.
D)Both are identical.
E)none of the above
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Multiple Choice
Q 130Q 130
Which of the following is most likely to have the weakest induced dipole-induced dipole interaction?
A)Cl2
B)Br2
C)F2
D)I2
E)All of the above have the same interactions.
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Multiple Choice
Q 131Q 131
Which of the following would have the highest boiling point?
A)Cl2
B)Br2
C)F2
D)I2
E)not enough information given
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Multiple Choice
Q 132Q 132
Which of the following would have the lowest melting point?
A)CCl4
B)CBr4
C)CF4
D)CI4
E)not enough information given
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Multiple Choice
Q 133Q 133
Which of the following would have the highest boiling point?
A)C6H14
B)C8H18
C)C10H22
D)C12H26
E)not enough information given
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Multiple Choice
Q 134Q 134
Which of the following would have the smallest number of induced dipole-induced dipole interactions?
A)C6H14
B)C8H18
C)C10H22
D)C12H26
E)not enough information given
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Multiple Choice
Q 135Q 135
Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18)have only limited solubility in water?
A)dipole-dipole
B)induced dipole-induced dipole
C)dipole-induced dipole
D)ion-dipole
E)Both A and B
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Multiple Choice
Q 136Q 136
Which of the following intermolecular forces best describes why molecules like sucrose (which has many OH groups)are very water soluble?
A)dipole-dipole
B)induced dipole-induced dipole
C)dipole-induced dipole
D)ion-dipole
E)hydrogen bonding
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Multiple Choice
Q 137Q 137
Which of the following intermolecular forces best describes why molecules like CF3CF3 are soluble in liquid CO2?
A)dipole-dipole
B)induced dipole-induced dipole
C)dipole-induced dipole
D)ion-dipole
E)hydrogen bonding
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Multiple Choice
Q 138Q 138
The charges with sodium chloride are all balanced-for every positive sodium ion there is a corresponding negative chloride ion.Since its charges are balanced,how can sodium chloride be attracted to water,and vice versa?
A)Dispersion forces come into play as the sodium chloride and water come into close proximity.
B)Hydrogen bonding in water allows the sodium chloride molecule to be attracted to the water molecule.
C)As a water molecule gets close to the sodium chloride it can distinguish the various ions and it is thus attracted to an individual ion by ion-dipole forces.
D)This is not a matter of attraction.Sodium chloride dissolves in water because water provides a medium in which the individual sodium and chloride ions can disperse.
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Multiple Choice
Q 139Q 139
Why is calcium fluoride,Ca ,a high melting point crystalline solid while stannic chloride, ,is a volatile liquid?
A)There is no theory to predict the physical property of melting point.Melting point temperatures are empirically determined.
B)Actually,we would predict these results to be the opposite.Since each metal is combined with a group 17 halogen,the heavier metal (tin)combination should have the higher melting point.
C)Ca is a small,linear,non-polar molecule,while is a huge tetrahedral structure.Therefore the bonds in calcium fluoride tend to give it a higher melting point temperature.
D)Ionic compounds formed by elements on opposite sides of the periodic table,like ,tend to have higher melting points than more covalently bonded structures,like
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Multiple Choice
Q 140Q 140
Why are ion-dipole attractions stronger than dipole-dipole attractions?
A)The chemical bond in an ion-dipole molecule is similar also a covalent bond.
B)The magnitude of the electric charge associated with an ion is much greater.
C)Dipole areas are subject to changing from positive to negative regions on the molecule.
D)Like charge (dipole)does not attract like charge (another dipole).
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Multiple Choice
Q 141Q 141
Chlorine, ,is a gas at room temperature,but bromine, ,is a liquid.Explain.
A)Chlorine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable.
B)Bromine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable.
C)The smaller chlorine molecules are able to pack together in a tighter physical orientation.
D)The bromine ions are held together by ionic bonds.
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Multiple Choice
Q 142Q 142
Plastic wrap is made of nonpolar molecules and is able to stick well to polar surfaces,such as glass,by way of dipole/induced dipole molecular attractions.How is it that plastic wrap also sticks to itself so well?
A)by way of dipole-dipole molecular attractions
B)by way of dipole-induced dipole molecular attractions
C)Ions are formed as the plastic rubs against itself.
D)by way of induced dipole-induced dipole molecular attractions
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Multiple Choice
Q 143Q 143
Dipole-induced dipole forces of attraction exist between water and gasoline,and yet these two substances do not mix because water has such a strong attraction for itself.Which of the following compounds might best help to make these two substances mix into a single liquid phase?
A)the molecule on the far left because the O-H bond is polar and the carbon and hydrogen bonds are nonpolar
B)the molecule in the middle because when the salts mix into the water,it will help separate the water and decrease the attraction for itself
C)The molecule on the right will form attractions with the polar ends of the water,allowing the gasoline a chance to mix with the water.
D)All of these molecules would be equally effective at increasing the mixing of gasoline and water.
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Multiple Choice
Q 144Q 144
How are oxygen molecules attracted to water molecules?
A)The attraction between oxygen and water molecules is a classic example of dipole-dipole interaction.
B)The hydrogen bonding in water causes the attraction of the oxygen atoms in the molecule to water.
C)As a water molecule is brought close to an oxygen molecule an induced dipole results in the molecule causing the attraction.
D)The attraction of oxygen and water molecules for one another is part of the common atom effect.Since both molecules contain oxygen,there is a built-in attraction.
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Multiple Choice
Q 145Q 145
List the following compounds in order of increasing boiling point: , , , .
A) , , ,
B) , , ,
C) , , ,
D) , , ,
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Multiple Choice
Q 146Q 146
Why is the surface area of a gecko's foot so extensive?
A)A gecko,like all amphibians,needs extensive surface area under foot for stability on land as well as mobility in water.
B)A gecko's foot acts like a large dipole and thus allows for ion-dipole interaction in water.
C)The greater the surface area the greater the number of induced dipole-induced dipole forces of attraction that can occur between the gecko's foot and the surface.
D)The extensive surface area,once charged by the gecko's body,allows for the dipole-dipole attraction of every contact surface.
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Multiple Choice
Q 147Q 147
Consider the boiling points of the following compounds and their solubilities in room-temperature water.Why does the solubilities in water go down as the boiling points of these alcohols go up.
A)Larger molecules are less attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions.
B)As the boiling increases,it is more difficult to keep the alcohol from evaporating out of solution.
C)As the boiling point increases,the size of the alcohol molecules decreases.
D)Larger molecules are more attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions.
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Multiple Choice
Q 148Q 148
The boiling point of 1,4-butanediol is 230°C.Would you expect this compound to be soluble or insoluble in room-temperature water?
A)Since there are no polar areas on this molecule,it is insoluble in water at room temperature.
B)A high boiling point means that the substance interacts with itself quite strongly.Therefore this molecule is not soluble in water.
C)Since there are polar areas on this molecule,it is insoluble in water at room temperature.
D)Water would be attracted to both ends of 1,4 butanediol,and it is infinitely soluble in water.
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Multiple Choice
Q 149Q 149
Two chemical structures are shown,one of a typical gasoline molecule and the other of a typical motor oil molecule.Which is which? Base your reasoning not on memorization but rather upon what you know about molecular interactions and the various physical properties of gasoline and motor oil.
A)Structure A represents the gas molecule because there are more bonds to gain energy from,giving it a higher energy content than oil.
B)Structure A represents motor oil,illustrating a molecule with greater induced dipole-induced dipole molecular interactions thus,the molecules are strongly attracted to one another.
C)Structure B represents the oil molecule.Because oil molecules are smaller,they can compact closer together,giving the appearance of a thicker solution than gasoline.
D)Structure B represents crude oil which is processed to generate longer molecules of gasoline to prevent toxic vapors from harming consumers.
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Multiple Choice
Q 150Q 150
Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds?
A)Ionic bonds are so much stronger than the molecular attractions between covalently bonded compounds.
B)Covalent bonds are not as strong as ionic bonds.
C)As a solid,salts have a very organized crystalline structure which takes a lot of energy to break apart.
D)Most covalent compounds have at least one weak bond in their structure that is easily broken when heat is added.
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Multiple Choice