Question 1

Which of the following oxides will give the most acidic solution when dissolved in water? A)MgO B)Al ₂O ₃ C)Cl ₂O D)SrO E)H ₂O ₂

Accepted Answer

Cl₂O forms HClO when dissolved in water, which is a weak acid, making the solution acidic. MgO and SrO are basic oxides, Al₂O₃ is amphoteric, and H₂O₂ doesn't form an acidic solution.

Question 2

Which of the following will have the highest boiling point? A)O ₂ B)Cl ₂ C)Br ₂ D)I ₂ E)Xe

Accepted Answer

The boiling point of substances increases with the size and mass of the molecules or atoms. Among the given options, iodine (I) is the largest and heaviest, leading to the highest boiling point due to stronger London dispersion forces.

Question 3

Which of the following atoms has the smallest volume?
A)Ba
B)Cs
C)Sr
D)Rb
E)I

Accepted Answer

As we move down a group in the periodic table, the atomic radius increases due to the addition of more electron shells. Therefore, the largest element in the group will have the largest atomic radius and volume. Among the given options, iodine (I) is located at the bottom of group 17, and therefore it should have the largest atomic radius and volume.

Question 4

Hydrogen forms metallic (interstitial) hydrides with the d and f transition elements. Which of the following statements is correct?
A)These substances have distinct stoichiometric formulas like ionic hydrides.
B)Hydrogen forms bonds with the metals by donating its electron to the valence band of the metal.
C)Hydrogen molecules and atoms occupy holes within the crystal structure of the metal.
D)These substances are useful catalysts.
E)These hydrides are stabilized by hydrogen bonding forces.

Accepted Answer

Metallic (interstitial) hydrides are formed when hydrogen molecules and atoms occupy holes within the crystal structure of the metal. They do not have distinct stoichiometric formulas like ionic hydrides, nor do they form bonds with the metals by donating their electron to the valence band of the metal. While some metallic hydrides may be useful catalysts, this is not a universal property. Additionally, these hydrides are not stabilized by hydrogen bonding forces.

Question 5

The smallest ionization energies are found in the __________ __________ region of the periodic table.
A)upper right
B)upper left
C)lower right
D)lower left
E)transition element ( d-block)

Accepted Answer

The smallest ionization energies are found in the lower left region of the periodic table because elements in this area have larger atomic radii and their outer electrons are further from the nucleus, making them easier to remove.

Question 6

Although the periodic table is organized according to the atomic numbers of the elements, chemists are more interested in the arrangement of the electrons for their studies. Which of the following statements about the electron configurations and their quantum numbers is correct?
A)The size of an atom is associated with the angular momentum quantum number.
B)The valence electrons of atoms in a particular group have the same principal and angular momentum quantum numbers.
C)The valence electrons of atoms in a particular group have the same angular momentum quantum number but have different principal quantum numbers.
D)Quantum numbers for the electrons tell us little about the relative energies of the electrons.
E)None of these choices are correct.

Accepted Answer

The valence electrons of atoms in a particular group in the periodic table have the same angular momentum quantum number (l), which determines the shape of the electron cloud, but they have different principal quantum numbers (n), which indicates the energy level or shell that the electron occupies. This is why elements in the same group have similar chemical properties; their valence electrons are in orbitals of the same type but at different energy levels as you move down the group.

Question 7

What are the products of the reaction of potassium hydride and water? KH(s) + H₂O(l) → A)K( s)+ H ₂( g)+ OH ⁻( aq) B)K( s)+ H ₂( g)+ O ₂( g) C)KOH( s)+ O ₂( g) D)K ⁺( aq)+ H ₂( g)+ O ₂( g) E)K ⁺( aq)+ H ₂( g)+ OH ⁻( aq)

Accepted Answer

When potassium hydride is added to water, it will react to form potassium hydroxide and hydrogen gas. The balanced equation for the reaction is:

KH(s) + H2O(l) → KOH(s) + H2(g)

Option E is the best choice as it includes the correct products, namely potassium ions (K+), water (H2O), hydrogen gas (H2), and hydroxide ions (OH-). Option A, B, C, and D are incorrect as they include products that are not formed in this reaction.

Question 8

Which one of the following elements is likely to exhibit the most violent and rapid reaction with water? A)Na B)Rb C)Mg D)Sr E)Cl ₂

Accepted Answer

Rb (rubidium) is in Group 1 of the periodic table, which means it has only one valence electron that it wants to get rid of. This makes it highly reactive with water, leading to a violent and rapid reaction. Mg (magnesium) and Sr (strontium) are both in Group 2 and are less reactive than Group 1 elements. Na (sodium) is also in Group 1 but is less reactive than Rb. Cl (chlorine) is a non-metal and does not react violently with water.

Question 9

Bromine will form compounds with each of the other elements in Period 4 of the periodic table. How does the type of bonding in the compounds change as one moves from potassium bromide to selenium bromide?
A)Ionic to polar covalent
B)Polar covalent to ionic
C)Polar covalent to non-polar covalent
D)Coordinate covalent to polar covalent
E)None of these choices are correct.

Accepted Answer

As one moves from potassium (a metal) to selenium (a nonmetal) in Period 4 of the periodic table, the type of bonding changes from ionic (between metals and nonmetals) to polar covalent (between nonmetals with different electronegativities).

Question 10

What are the products of the following reaction of strontium hydride and water? SrH₂(s) + H₂O(l) → A)Sr ²⁺( aq)+ H ₂( g)+ O ₂( g) B)Sr ²⁺( aq)+ H ₂( g)+ OH ⁻( aq) C)Sr( s)+ H ₂( g)+ OH ⁻( aq) D)Sr( s)+ H ₃O ⁺( aq) E)None of these choices are correct.

Accepted Answer

When strontium hydride (SrH2) reacts with water, it forms strontium hydroxide (Sr(OH)2) and hydrogen gas (H2). The balanced equation is:

SrH2 + 2H2O → Sr(OH)2 + 2H2

However, in this question, SrHS is used instead of SrH2. This is a bit unusual, as SrHS is not a commonly known compound. However, we can still use the same general reaction for our prediction.

So, SrHS and water should form strontium hydroxide and hydrogen gas. The only answer choice that includes both of these products is B. Additionally, it also includes hydrogensulfide gas (H2S), which is likely formed due to the presence of impurities in the SrHS sample.

Question 11

Which of the following pairs of elements will form the longest single bond?
A)C, F
B)C, N
C)C, S
D)C, O
E)C, H

Accepted Answer

The length of a single bond between two atoms generally increases with the size of the atoms involved. Among the given options, sulfur (S) is the largest atom when compared to fluorine (F), nitrogen (N), oxygen (O), and hydrogen (H). Therefore, a bond between carbon (C) and sulfur (S) would be the longest due to the larger size of sulfur.

Question 12

Which of the following statements about the effective nuclear charge, Z_eff, is correct? A)Z _eff increases with the size of the atom. B)Z _eff decreases across a period and increases down a group. C)Z _eff increases across a period and is relatively constant down a group. D)Z _effincreases as the value of the principal quantum number increases. E)Z _eff is greater for hydrogen than for any other element.

Accepted Answer

The effective nuclear charge, Z_eff, is the net positive charge experienced by an electron in an atom. It takes into account the attractive force of the nucleus and the repulsive force of the electrons in the same electron shell. Across a period, the number of protons in the nucleus increases, which increases the attractive force on the electrons. At the same time, the number of electrons in the same shell also increases, which increases the repulsive force. As a result, the effective nuclear charge increases across a period. Down a group, the number of electron shells increases, which shields the outer electrons from the attractive force of the nucleus. As a result, the effective nuclear charge remains relatively constant down a group. Therefore, option C is correct: Z_eff increases across a period and is relatively constant down a group.

Question 13

Which of the following ions and atoms has the greatest radius? A)Se ²⁻ B)Br ⁻ C)Rb ⁺ D)Sr ²⁺ E)Kr

Accepted Answer

The answer of Which of the following ions and atoms...

Question 14

Which of the following oxides will give the most basic solution when dissolved in water? A)SO ₂ B)CO ₂ C)K ₂O D)P ₄O ₁₀ E)SO ₃

Accepted Answer

When oxides dissolve in water, they can either form acidic or basic solutions. Basic solutions are created when the oxide reacts with water to form hydroxide ions (OH^-), which increase the pH of the solution. 
Out of the given options, K2O is the most basic oxide because it belongs to the Group 1 (alkali metals) which are known to form very basic solutions when dissolved in water.

Question 15

Select the element with the highest first ionization energy.
A)Mg
B)Ca
C)Ba
D)Ra
E)K

Accepted Answer

The answer of Select the element with the highest first...

Question 16

Select the element with the lowest first ionization energy.
A)Se
B)S
C)Sn
D)Sr
E)H

Accepted Answer

Sr (Strontium) has the lowest first ionization energy among the options given. This is because it is located further down the periodic table in Group 2, indicating it has more electron shells and the outer electrons are further from the nucleus, making them easier to remove compared to the other elements listed.

Question 17

Which of the following pure substances will not participate in hydrogen bonding? A)CH ₃NH ₂ B)CH ₃CH ₂OCH ₂CH ₃ C)CH ₃CH ₂OH D)HF E)H ₂O ₂

Accepted Answer

CH₃CH₂OCH₂CH₃ (an ether) does not have hydrogen atoms bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine, which are necessary for hydrogen bonding.

Question 18

The largest electronegativities are found in the __________ __________ region of the periodic table.
A)upper left
B)upper right
C)lower left
D)lower right
E)transition element ( d-block)

Accepted Answer

Electronegativity increases as you move towards the upper right corner of the periodic table, as the nucleus of the atom has a greater positive charge and a smaller atomic radius, making it more attractive to electrons.

Question 19

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. The ionic radius for Na⁺ is 102 pm and for Cl⁻ is 181 pm. In going from Na to Cl in Period 3, why does the atomic radius decrease while the ionic radius increases? A)The inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do. B)The inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion. C)The outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do. D)The outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do. E)Monatomic ions are bigger than the atoms from which they are formed.

Accepted Answer

The outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do.

Question 20

Which of the following elements has the lowest electronegativity?
A)Al
B)S
C)Mg
D)In
E)Ba

Accepted Answer

Electronegativity increases from left to right in a period and decreases from top to bottom in a group. Among the given options, Ba is located at the bottom left corner of the periodic table and therefore has the lowest electronegativity.

Quiz 14: Periodic Patterns in the Main-Group Elements

Which of the following oxides will give the most acidic solution when dissolved in water?

Which of the following will have the highest boiling point?

Which of the following atoms has the smallest volume?

Hydrogen forms metallic (interstitial) hydrides with the d and f transition elements. Which of the following statements is correct?

The smallest ionization energies are found in the region of the periodic table.

Although the periodic table is organized according to the atomic numbers of the elements, chemists are more interested in the arrangement of the electrons for their studies. Which of the following statements about the electron configurations and their quantum numbers is correct?

What are the products of the reaction of potassium hydride and water? KH(s) + H₂O(l) →

Which one of the following elements is likely to exhibit the most violent and rapid reaction with water?

Bromine will form compounds with each of the other elements in Period 4 of the periodic table. How does the type of bonding in the compounds change as one moves from potassium bromide to selenium bromide?

What are the products of the following reaction of strontium hydride and water? SrH₂(s) + H₂O(l) →

Which of the following pairs of elements will form the longest single bond?

Which of the following statements about the effective nuclear charge, Z_eff, is correct?

Which of the following ions and atoms has the greatest radius?

Which of the following oxides will give the most basic solution when dissolved in water?

Select the element with the highest first ionization energy.

Select the element with the lowest first ionization energy.

Which of the following pure substances will not participate in hydrogen bonding?

The largest electronegativities are found in the region of the periodic table.

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. The ionic radius for Na⁺ is 102 pm and for Cl⁻ is 181 pm. In going from Na to Cl in Period 3, why does the atomic radius decrease while the ionic radius increases?

Which of the following elements has the lowest electronegativity?