Deck 2: Atoms, Molecules, and Ions

Question 1

An anion is defined as

A)a charged atom or group of atoms with a net negative charge.
B)a stable atom.
C)a group of stable atoms.
D)an atom or group of atoms with a net positive charge.

Answer 1

a charged atom or group of atoms with a net negative charge.

Question 2

Which one of the following elements is most likely to form a 2- ion?

A)scandium
B)selenium
C)silicon
D)strontium
E)iodine

Answer 2

selenium

Question 3

How many neutrons are there in an atom of uranium whose mass number is 235?

A)92
B)143
C)235
D)238
E)327

Answer 3

143

Question 4

A magnesium ion, Mg²⁺, has

A)12 protons and 13 electrons.
B)24 protons and 26 electrons.
C)12 protons and 10 electrons.
D)24 protons and 22 electrons.
E)12 protons and 14 electrons.

Question 5

When J. J. Thomson discovered the electron, what physical property of the electron did he measure?

A)its charge, e
B)its charge-to-mass ratio, e/m
C)its temperature, T
D)its mass, m
E)its atomic number, Z

Question 6

An oxide ion, O^2-, has:

A)8 protons and 10 electrons
B)10 protons and 8 electrons
C)8 protons and 9 electrons
D)8 protons and 7 electrons
E)10 protons and 7 electrons

Question 7

The elements in a column of the periodic table are known as

A)metalloids.
B)a period.
C)noble gases.
D)a group.
E)nonmetals.

Question 8

Which of the following scientists developed the nuclear model of the atom?

A)John Dalton
B)Robert Millikan
C)J. J. Thomson
D)Henry Moseley
E)Ernest Rutherford

Question 9

Which one of the following elements is most likely to form a 2+ ion?

A)beryllium
B)carbon
C)fluorine
D)oxygen
E)sodium

Question 10

An aluminum ion, Al³⁺, has:

A)13 protons and 13 electrons
B)27 protons and 24 electrons
C)16 protons and 13 electrons
D)13 protons and 10 electrons
E)10 protons and 13 electrons

Question 11

Which of the following elements is most likely to be a good conductor of electricity?

A)N
B)S
C)He
D)Cl
E)Fe

Question 12

In a cathode ray tube

A)electrons pass from the anode to the cathode.
B)electrons pass from the cathode to the anode.
C)protons pass from the anode to the cathode.
D)protons pass from the cathode to the anode.

Question 13

An atom of the isotope chlorine-37 consists of how many protons, neutrons, and electrons? (p = proton, n = neutron, e = electron)

A)17 p, 18.45 n, 17 e
B)17 p, 20 n, 7 e
C)17 p, 20 n, 17 e
D)17 p, 37 n, 17 e
E)20 p, 17 n, 20 e

Question 14

Rutherford's experiment with alpha particle scattering by gold foil established that

A)protons are not evenly distributed throughout an atom.
B)electrons have a negative charge.
C)electrons have a positive charge.
D)atoms are made of protons, neutrons, and electrons.
E)protons are 1840 times heavier than electrons.

Question 15

Which one of the following is an ion?

A)B³⁺
B)NaCl
C)He
D)(¹⁴C)
E)none of the above

Question 16

Give the number of protons (p), electrons (e), and neutrons (n)in one atom of nickel-62.

A)28 p, 28 e, 28 n
B)28 p, 28 e, 34 n
C)28 p, 28 e, 62 n
D)62 p, 28 e, 28 n
E)62 p, 62 e, 28 n

Question 17

Atoms of the same element with different mass numbers are called

A)ions.
B)neutrons.
C)allotropes.
D)chemical families.
E)isotopes.

Question 18

The scientist who determined the magnitude of the electric charge of the electron was

A)John Dalton.
B)Robert Millikan.
C)J. J. Thomson.
D)Henry Moseley.
E)R. Chang.

Question 19

Two isotopes of an element differ in their

A)symbol.
B)atomic number.
C)atomic mass.
D)number of protons.
E)number of electrons.

Question 20

How many protons are there in an atom of uranium whose mass number is 235?

A)92
B)143
C)235
D)238
E)327

Question 21

Which is the correct formula for copper(II)phosphate?

A)Cu₂PO₄
B)Cu₃(PO₄)₂
C)Cu₂PO₃
D)Cu(PO₄)₂
E)Cu(PO₃)₂

Question 22

How many protons and electrons are present in one Br^- ion?

A)35 p, 35 e
B)80 p, 81 e
C)35 p, 34 e
D)35 p, 36 e
E)80 p, 34 e

Question 23

Which of the following is the formula for hydrobromic acid?

A)KBr
B)HBr
C)HBrO
D)HBrO₂
E)HBrO₃

Question 24

Which pair of elements would be most likely to form an ionic compound?

A)P and Br
B)Zn and K
C)F and Al
D)C and S
E)Al and Rb

Question 25

The formula for calcium phosphate is

A)CaPO₄.
B)Ca₃(PO₄)₂.
C)Ca₂(PO₄)₃.
D)Ca₃P₂.
E)Ca₃(PO₃)₂.

Question 26

Predict the formula for the binary compound formed between barium and phosphorus.

A)BaP
B)Ba₂P
C)BaP₂
D)Ba₂P₃
E)Ba₃P₂

Question 27

An iron(II)ion has:

A)24 electrons and a charge of 2+
B)24 electrons and a charge of 2-
C)26 electrons and a charge of 2+
D)28 electrons and a charge of 2+
E)28 electrons and a charge of 2-

Question 28

What is the formula for the ionic compound formed by magnesium and iodine?

A)MgI
B)Mg₂I
C)MgI₂
D)MgI₃
E)Mg₃I

Question 29

Which of the following pairs of elements would be most likely to form an ionic compound?

A)P and Br
B)Cu and K
C)C and O
D)O and Zn
E)Al and Rb

Question 30

A phosphide ion has:

A)10 protons and 13 electrons
B)12 protons and 15 electrons
C)15 protons and 15 electrons
D)15 protons and 18 electrons
E)18 protons and 21 electrons

Question 31

What is the formula for the binary compound formed by potassium and nitrogen?

A)KN
B)K₂N
C)NK₂
D)K₃N
E)NK₃

Question 32

What is the formula for the ionic compound formed by calcium ions and nitrate ions?

A)Ca₃N₂
B)Ca(NO₃)₂
C)Ca₂NO₃
D)Ca₂NO₂
E)CaNO₃

Question 33

What is the formula for the ionic compound formed by calcium and selenium?

A)CaSe
B)Ca₂Se
C)CaSe₂
D)Ca₃Se
E)CaSe₃

Question 34

Name the binary compound formed between barium and phosphorus.

A)barium phosphorus
B)barium phosphide
C)barium phosphate
D)barium diphosphate
E)barium triphosphide

Question 35

The chemical name for ClO₂^- is chlorite ion. Therefore, the name of HClO₂ is

A)hydrochloric acid.
B)chloroform.
C)hydrogen dioxychloride.
D)chlorous acid.
E)chloric acid.

Question 36

Given that the ion ClO₃^- is named chlorate, what is the ion ClO₄^- named?

A)chloride
B)chlorite
C)hypochlorite
D)perchlorite
E)perchlorate

Question 37

The chemical name for ClO₃^- is chlorate ion. Therefore, the name of HClO₃ is

A)hydrochloric acid.
B)chloroform.
C)hydrogen trioxychloride.
D)chlorous acid.
E)chloric acid.

Question 38

The correct name for NH₄NO₃ is

A)ammonium nitrate.
B)ammonium nitrogen trioxide.
C)ammonia nitrogen oxide.
D)hydrogen nitrogen oxide.
E)hydrogen nitrate.

Question 39

The formula for sodium sulfide is

A)NaS.
B)K₂S.
C)NaS₂.
D)Na₂S.
E)SeS.

Question 40

The formula for magnesium sulfate is

A)MnS.
B)MgS.
C)MnSO₃.
D)MgSO₄.

Question 41

The Stock system name for CrO₃ is:

A)chromium oxide
B)chromium(II)oxide
C)chromium(III)trioxide
D)chromium(III)oxide
E)chromium(VI)oxide

Question 42

The correct name for CuSO₄·5H₂O is

A)copper sulfate acid.
B)copper sulfate pentahydrate.
C)copper(II)sulfate acid.
D)copper(II)sulfate pentahydrate.
E)copper(V)sulfate hydrate.

Question 43

The mineral manganosite is a compound of manganese-55 and oxygen-16. If 77% of the mass of manganosite is due to manganese, what is the empirical formula of manganosite?

A)MnO
B)Mn₂O
C)Mn₂O₂
D)MnO₂
E)none of these

Question 44

The Stock system name for Co₂(SO₃)₃ is:

A)cobalt sulfate
B)cobalt(II)sulfite
C)cobalt(II)sulfate
D)cobalt(III)sulfite
E)cobalt(III)sulfate

Question 45

The chemical formula for iron(II)nitrate is:

A)Fe₂(NO₃)₃
B)Ir(NO₂)₂
C)Fe₂N₃
D)Fe(NO₃)₂
E)Fe(NO₂)₂

Question 46

The correct name for Ba(OH)₂ is

A)barium hydrogen oxide.
B)boron hydroxide.
C)barium hydrate.
D)beryllium hydroxide.
E)barium hydroxide.

Question 47

The mineral pyrolusite is a compound of manganese-55 and oxygen-16. If 63% of the mass of pyrolusite is due to manganese, what is the empirical formula of pyrolusite?

A)MnO
B)Mn₂O
C)Mn₂O₂
D)MnO₂
E)none of these

Question 48

The Stock system name for As₂S₅ is

A)arsenic(V)sulfide.
B)diarsenic pentasulfide.
C)arsenic(III)sulfide.
D)arsenic(V)sulfate.
E)diarsenic sulfate.

Question 49

Which of the following elements is chemically similar to magnesium?

A)sulfur
B)calcium
C)iron
D)nickel
E)potassium

Question 50

Which of the following elements is chemically similar to oxygen?

A)sulfur
B)calcium
C)iron
D)nickel
E)sodium

Question 51

Which of the following elements is chemically similar to potassium?

A)calcium
B)arsenic
C)phosphorus
D)cerium
E)cesium

Question 52

The correct name for KHCO₃ is

A)calcium bicarbonate.
B)calcium carbonate.
C)potassium carbonate.
D)calcium hydrogen carbon trioxide.
E)potassium hydrogen carbonate.

Question 53

The Stock system name for Mn₂O₇ is

A)dimanganese heptaoxide.
B)magnesium oxide.
C)manganese(VII)oxide.
D)manganese(II)oxide.
E)manganese(III)oxide.

Question 54

The straight chain hydrocarbon that contains six carbon atoms is

A)propane.
B)butane.
C)pentane.
D)hexane.
E)heptane.

Question 55

The mineral hausmannite is a compound of manganese-55 and oxygen-16. If 72% of the mass of hausmannite is due to manganese, what is the empirical formula of hausmannite?

A)MnO
B)Mn₃O
C)Mn₃O₄
D)Mn₄O₃
E)MnO₃

Question 56

The mineral orpiment, having the empirical formula As₂S₃, was used in ancient times as a cosmetic. What mass of arsenic is present in 5.0 g of orpiment? [Given: naturally occurring arsenic is all arsenic-75; assume that all naturally occurring sulfur is sulfur-32 (only approximately true)]

A)0.61 g
B)3.0 g
C)1.5 g
D)2.0 g
E)3.5 g

Question 57

Which is the correct formula for lead(IV)chloride?

A)Pb₄Cl
B)PbCl₂
C)PbCl₃
D)PbCl₄
E)Pb₂Cl₄

Question 58

Consistent with vanadium being a transition metal, the name for VSO₄ should be

A)vanadium sulfide.
B)vanadium (I)sulfite.
C)vanadium (I)sulfate.
D)vanadium (II)sulfate.
E)vanadium sulfur tetraoxide.

Question 59

Give the formula for cobalt(II)chlorate dihydrate:

A)CoCl₂·2H₂O
B)CoClO₃(H₂O)₂
C)Co(ClO₃)₂(H₂O)₂
D)Co(ClO₃)₂·2H₂O
E)Co₂(ClO₃)₃·2H₂O

Question 60

Zircon is a mineral with the empirical formula ZrSiO₄. If all the zirconium is ⁹⁰Zr, all the silicon is ²⁸Si, and all the oxygen is ¹⁶O, what mass of oxygen is present in 10. g of zircon?

A)0.88 g
B)1.2 g
C)1.8 g
D)3.5 g
E)5.4 g

Question 61

Use the periodic table above to show where the alkaline earth metals are located.

Question 62

How many protons are there in one atom of magnesium?

Question 63

Use the periodic table above to show where the metals are located.

Question 64

Use the periodic table above to show where the halogen elements are located.

Question 65

Use the periodic table above to show where the metalloids are located.

Question 66

Define the term molecule.

Question 67

What is the law of conservation of mass?

Question 68

What are the three subatomic particles that are important in chemistry?

Question 69

What are the three types of radiation produced by the decay of substances like uranium?

Question 70

Use the periodic table above to show where the nonmetals are located.

Question 71

Use the periodic table above to show where the noble gases are located.

Question 72

Define ion.

Question 73

In the early 1900s, Ernest Rutherford performed an experiment with gold foil targets and alpha particles to probe the structure of the atoms. He observed that most of these alpha particles penetrated the foil undeflected. Realizing that atoms are electrically neutral (that is, they have equal numbers of protons and electrons)and that the mass of a proton is significantly greater than the mass of an electron, use Rutherford's data to propose a structural model of an atom.

Question 74

What are the seven elements that naturally occur as diatomic molecules?

Question 75

Use the following to answer questions 70-76:
Use the periodic table above to show where the alkali metals are located.

Question 76

How many protons are there in one atom of xenon?

Question 77

How many protons are there in one atom of nickel?

Question 78

How many protons are there in one atom of uranium?

Question 79

Describe the contributions of Marie Curie.

Question 80

How many electrons, protons, and neutrons does an iron-55 atom have?