1

Unit 3 Practice QuestionsI. Ionic Bonding

Questions 1-3 refer to the following:

(A) X+

(B) X+2

(C) X+3

(D) XO3-2

(E) XO4-2

1. A type of ion found in sodium acetate2. A type of ion found in aluminum oxide3. A type of ion found in potassium phosphate

2

Questions 1-2 refer to the following:

(A) 1(B) 7(C) 9(D) 10(E) 14

1. The atomic number of an atom with an electron dot arrangement similar to iodine

2. The number of atoms represented in the formula Al(OH)3

3

Questions 1-4 refer to the following:

(A) Na+

(B) Al(C) F(D) Ti(E) Br--

1. Has 7 valence electrons2. Has the electron configuration 1s22s22p63s23p1

3. Has the same electron configuration as a neon atom

4. Has valence electrons in d orbitals

4

Questions 1-5 refer to the following:

(A) Ca+ and K(B) H+ and He(C) Cl- and F(D) O- and S+

(E) Na+ and O--

1. Difference of 6 electrons2. Same number of electrons3. Difference of 9 electrons4. Difference of 2 electrons5. Difference of 1 electron

5

I

Molten sodium chloride is a good electrical conductor

II

Sodium chloride in the molten state allows ions to move freely

Sodium chloride is an example of ionic bonding

Sodium and chlorine have the same electronegativity

BECAUSE

BECAUSE

6

I

An ionic solid is a good conductor of electricity

II

An ionic solid is composed of positive and negative ions joined together in a lattice structure held together by electrostatic forces

When a chlorine atom gains an electron, it becomes a positively charged ion

A neutral atom has equal numbers of protons and electrons

BECAUSE

BECAUSE

7

I

Crystals of sodium chloride go into solution in water as ions

II

The sodium ion has a 1+ charge and the chloride ion has a 1- charge and they are hydrated by the water molecules

For an element with an atomic number of 17, the most probable oxidation number (charge) is +1

The outer energy level of the halogen family has a tendency to add one electron to itself

BECAUSE

BECAUSE

8

I

The ionic bond is the strongest bond

II

Ionic bonds have electrostatic attraction due to the loss and gain of electrons

Atom A with 7 valence electrons forms AB2 with atom B with two valence electrons

B donates its electrons to fill the outer shell of A

BECAUSE

BECAUSE

9

I

MgO has a high melting point

II

Highly charged ions result in strong ionic forces and high lattice energies

A solution of NaCl will conduct electricity

NaCl will not form ions in solution

BECAUSE

BECAUSE

10

The correct formula for calcium hydrogen sulfate is

(A) CaH2SO4

(B) CaHSO4

(C) Ca(HSO4)2

(D) Ca2HSO4

(E) Ca2H2SO4

11

Which sample below has its atoms arranged in a regular, geometric pattern?

(A) NaC2H3O2 (s)(B) H2O (l)(C) Ar (g)(D) NaCl (aq)(E) CH4 (g)

12

How many electrons does a 37Cl ion with a charge of -1 contain?

(A) 16(B) 17(C) 18(D) 37(E) 38

13

Which element is most likely represented by X in the oxygen-containing ion, XO4

-3?

(A) C(B) N(C) P(D) S(E) Cl

14

Which of the following is NOT true of the element sodium?

(A) It takes the oxidation state (charge) +1(B) It reacts with water to form a basic solution(C) It forms metallic bonds in its solid uncombined

form(D) It is found in nature as a diatomic gas(E) It reacts with a halogen to form an ionic salt

15

How many atoms are present in the formula KAl(SO4)2?

(A) 7(B) 9(C) 11(D) 12(E) 13

16

Which sample has atoms that are arranged in a regular geometric pattern?

(A) KCl (l)(B) NaC2H3O2 (s)(C) Fe (l)(D) NaCl (aq)(E) HCl (aq)

17

When an ionic compound is dissolved in water, the ions in solution can best be described as

(A) Hydrated molecules only(B) Dehydrated ions and molecules(C) Both hydrated molecules and hydrated ions(D) Neither hydrated ions nor hydrated molecules(E) Hydrated ions only

18

What is the chemical formula for iron(III) sulfate?

(A) Fe2SO4

(B) Fe3SO4

(C) Fe(SO4)3

(D) Fe2(SO4)3

(E) Fe2S3

19

The name of the compound MgBr2 is

(A) Manganese bromite(B) Manganese bromide(C) Magnesium bromite(D) Magnesium bromide(E) Magnesium dibromide

20

The anion S2- is called

(A) Sulfide(B) Sulfite(C) Sulphorous(D) Sulfuron(E) Sulfate

21

Element X forms the compounds XCl3 and X2O3. Element X would most likely belong to the group called

(A) Alkali metals(B) Alkaline earth metals(C) Group 13(D) Halogens(E) Noble gases

22

A nonmetal (X) reacts with a metal (M) to give the formula M2X. Which pairing below is most like elements represented by M and X?

(A) Ca and N(B) Li and S(C) Si and O(D) Rb and F(E) Mg and Cl

23

In the Lewis dot structure X: , what is the predictable oxidation number (charge)?

(A) +1(B) -1(C) +2(D) -2(E) +3

24

Which of the following compounds would be expected to have the greatest lattice binding energy?

(A) LiNO3

(B) LiF(C) KI(D) NH4Br(E) CsNO3

25

Which of the following is true regarding an Ne atom with a mass number of 20 and an O2- ion with a mass number of 16?

(A) They contain the same number of protons(B) They contain the same number of neutrons(C) They contain the same number of protons plus

neutrons(D) They are isoelectronic(E) They are isomers

26

Which bonds are ionic?I. HClII. SClIII. CsF

(A) I only(B) III only(C) I and II only(D) II and III only(E) I, II and III

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II. Covalent Bonding

Questions 1-3 refer to the following:

(A) CH4

(B) CO2

(C) NH3

(D) N2

(E) O2

1. Forms hydrogen bonds2. Is polar3. Has a triple bond

28

I

A pi bond is formed between the lobes of adjacent p orbitals in the same plane of two atoms that contain only one electron each

II

Each of the two lobes of a single p orbital can hold two electrons of opposite spin

Ammonia (NH3) has a trigonal pyramidal molecular structure

Ammonia has a tetrahedral electron pair geometry with three atoms bonded to the central atom

BECAUSE

BECAUSE

29

I

Maximum repulsion between two electron pairs in a molecular compound will result in a linear structure

II

The VSEPR model says that like charges will orient themselves so as to diminish the repulsion between them

The structure of SO3 is shown by using more than one structural formula

SO3 is very unstable and resonates between these possible structures

BECAUSE

BECAUSE

30

I

The hybrid orbital form of carbon in acetylene (C2H2) is believed to be the sp form

II

C2H2 is a linear compound with a triple bond between the carbons

The weakest of the bonds between molecules are coordinate covalent bonds

Coordinate covalent bonds represent the weak attractive force of the electrons of one molecule for the positively charged nucleus of another

BECAUSE

BECAUSE

31

I

Water is a polar substance

II

The sharing of the bonding electrons in water is equal

Water is a good solvent for ionic and/or polar covalent substances

Water shows hydrogen bonding between oxygen atoms

BECAUSE

BECAUSE

32

I

The N-N bond distance in N2 is shorter than the N-N bond distance in N2H4

II

The atomic radius of H is smaller than the atomic radius of N

Elemental iodine has a higher boiling point than elemental bromine

Iodine forms stronger covalent bonds than bromine

BECAUSE

BECAUSE

33

I

The boiling point of H2O is higher than the boiling point of H2S

II

H2S has a greater molecular mass than H2O

Bromine has a higher boiling point than chlorine

Bromine has higher dispersion forces than chlorine

BECAUSE

BECAUSE

34

I

Some covalent bonds are polar in nature

II

Atoms of different electronegativities are unequal in the degree to which they attract electrons

A nonpolar molecule can have polar bonds

Polar bonds can be symmetrically arranged in a molecule so that there are no net poles

BECAUSE

BECAUSE

35

I

The bond in an O2 molecule is nonpolar

II

The oxygen atoms in an O2 molecule share the bonding electrons equally

BF3 has a tetrahedral geometry

The central B atom does not have a complete stable octet

BECAUSE

BECAUSE

36

I

Substances with hydrogen bonding tend to have unusually low boiling points

II

Extra energy is necessary to break the hydrogen bonds

CCl4 is a nonpolar compound

The dipole moments are canceled out

BECAUSE

BECAUSE

37

A tetrahedral molecule, XY4, would be formed if X were using the orbital hybridization

(A) p2

(B) s2

(C) sp(D) sp2

(E) sp3

38

Which of the elements below is most likely to form compounds in which it has an incomplete octet?

(A) B(B) C(C) N(D) O(E) F

39

Which substance has a polar covalent bond between its atoms?

(A) K3N(B) Ca3N2

(C) NaCl(D) F2

(E) NH3

40

Which molecule is a polar molecule?

(A) N2

(B) H2O(C) CH4

(D) CO2

(E) KCl

41

In which of the following compounds are hydrogen bonds between molecules the strongest?

(A) HF(B) HCl(C) HBr(D) HI(E) HAt

42

The compound PF5 is called

(A) Monophorofluoride(B) Phosphorus pentafluoride(C) Pentaphosphoro fluoride(D) Phosphorus tetrafluoride(E) Potassium pentafluoride

43

How many sigma and pi bonds are found in the following molecule?

H—C C—CH2—CH=CH2

(A) 6 sigma, 2 pi(B) 2 sigma, 6 pi(C) 10 sigma, 3 pi(D) 5 sigma, 3 pi(E) 11 sigma, 2 pi

44

Which of the following statements is false?

(A) H2 has just one sigma bond(B) HCl has just one sigma bond(C) H—C C—H has four pi and three sigma

bonds(D) CH2=CH2 has five sigma bonds and one pi bond(E) H2O has two sigma bonds and two lone pairs

45

How many pi bonds are there in a molecule of

N C—CH2—CH2—NH—CH=CH2

(A) 6(B) 4(C) 12(D) 10(E) 3

46

Which of the following species has a molecular shape most similar to that of ammonia, NH3?

(A) BH3

(B) H2O(C) H3O+

(D) CH4

(E) NH4+

47

Which compound below has a bent molecular geometry?

(A) H2SO4

(B) CH4

(C) CO2

(D) H2S(E) C2H2

48

Which compound of oxygen is most likely to contain an O-O bond?

(A) CO2

(B) NO2

(C) SO2

(D) H2O2

(E) TiO2

49

How many single bonds are in a molecule of carbon dioxide, CO2?

(A) None(B) One(C) Two(D) Three(E) Four

50

All of the following have covalent bonds EXCEPT

(A) HCl(B) CCl4

(C) H2O(D) CsF(E) CO2

51

Which of the following molecules is polar?

(A) BH3

(B) NF3

(C) C2H6

(D) SF6

(E) CCl4

52

The shape of a PCl3 molecule can be described as

(A) Bent(B) Trigonal pyramidal(C) Linear(D) Trigonal planar(E) Tetrahedral

53

Which of the following is a nonpolar molecule?

(A) CO2

(B) H2O(C) NH3

(D) NO(E) HI

54

The structure of SiO2 can best be described as

(A) Linear(B) Bent(C) Trigonal(D) Tetrahedral(E) Square

55

Which of the following molecules has a trigonal pyramidal geometry?

(A) BH3

(B) H2O(C) CH4

(D) NH3

(E) AlCl3

56

Which of these resembles the molecular structure of the water molecule?

(A) H—H—O, linear(B) H—O—H, bent, 30o angle(C) H—O—H, bent, 90o angle(D) H—O—H, bent, 105o angle(E) H—O—H, linear

57

The shape of a PCl3 molecule is described as

(A) Bent(B) Trigonal planar(C) Linear(D) Trigonal pyramidal(E) tetrahedral

58

The bond that includes an upper and a lower sharing of electron orbitals is called

(A) A pi bond(B) A sigma bond(C) A hydrogen bond(D) A covalent bond(E) An ionic bond

59

What is the structure associated with the BF3 molecule?

(A) Linear(B) Trigonal planar(C) Tetrahedron(D) Trigonal pyramidal(E) Bent

60

Which of these statements is the best explanation for the sp3 hybridization of carbon’s electrons?

(A) The new orbitals are one s orbital and three p orbitals

(B) The s electron is promoted to the p orbitals(C) The s orbital is deformed into a p orbital(D) Four new and equivalent orbitals are formed(E) The s orbital electron loses energy to fall back

into a partially filled p orbital

61

The intermolecular force that is most significant in explaining the variation of the boiling point of water from the boiling points of similarly structured molecules is

(A) Hydrogen bonding(B) Van der Waals forces(C) Covalent bonding(D) Ionic bonding(E) Coordinate covalent bonding

62

Which of the following properties can be attributed to water?

I. It has a permanent dipole moment attributed to its molecular structure

II. It is a very good conductor of electricityIII. It has polar covalent bonds with hydrogen

on opposite sides of the oxygen atom, so that the molecule is linear

(A) I only(B) III only(C) I and II only(D) II and III only(E) I, II and III

63

III. All Types of Bonding

Questions 1-3 refer to the following:

(A) Ionic substance(B) Metallic substance(C) Polar covalent molecule(D) Nonpolar covalent molecule(E) Aromatic organic molecule

1. Carbon tetrachloride2. Cesium chloride3. Hydrogen chloride

64

Questions 1-4 refer to the following:

(A) Ionic(B) Covalent(C) Polar covalent(D) Metallic(E) Hydrogen bonding

1. When the electronegativity difference between 2 atoms is 2

2. If two atoms are bonded in such a way that both members of the pair equally share one electron with the other

3. Which of the 5 choices is the weakest bond?4. If an electron is lost by one atom and completely

captured by another

65

Questions 1-3 refer to the following:

(A) Water(B) Hydrogen bromide(C) Iron(D) Argon(E) Sodium chloride

1. Hydrogen bonding2. Highly polar3. Dispersion forces

66

Questions 1-3 refer to the following:

(A) Ionic(B) Covalent(C) Polar covalent(D) Metallic(E) Hydrogen bonding

1. Bonding that explains water’s high boiling point2. If the sharing of an electron pair is unequal and the

atoms have an electronegativity difference of 1.4 to 1.6

3. If one or more valence electrons become detached from the atoms and migrate in a “sea” of free electrons among the positive metal ions

67

Questions 1-3 refer to the following:

(A) Hydrogen gas, H2

(B) Carbon monoxide, CO(C) Potassium, K(D) Aluminum oxide, Al2O3

(E) Bromine, Br2

1. Substance held together by metallic bonds2. Substance held together by ionic bonds3. Consists of polar molecules

68

Questions 1-4 refer to the following:

(A) Hydrogen bond(B) Ionic bond(C) Polar covalent bond(D) Nonpolar covalent bond(E) Metallic bond

1. The type of bond between atoms of potassium and chloride

2. The type of bond between the atoms in a nitrogen molecule

3. The type of bond between the atoms in CO2 (electronegativity difference = 1)

4. The type of bond between the atoms of calcium in a crystal of calcium

69

Questions 1-4 refer to the following:

(A) Ionic substance(B) Polar covalent substance(C) Nonpolar covalent substance(D) Amorphous substance(E) Metallic network

1. KCl (s)2. HCl (g)3. CH4 (g)4. Li (s)

70

Questions 1-4 refer to the following:

(A) Hydrogen bonding(B) Ionic bonding(C) Metallic bonding(D) Nonpolar covalent bonding(E) Polar covalent bonding

1. Holds a sample of barium iodide, BaI2, together2. Allows solids to conduct electricity3. Attracts atoms of hydrogen to each other in an H2

molecule4. Responsible for relatively low vapor pressure of

water

71

Questions 1-5 refer to the following:

(A) Hydrogen bonding(B) Ionic bonding(C) Network bonding(D) London dispersion force(E) Metallic bonding

1. Chiefly responsible for the relatively high boiling point of water

2. Is present in liquid oxygen3. Is primarily responsible for the hardness of

diamond4. Allows copper to conduct electricity5. Is present in solid KCl

72

I

Most atoms are less stable in the bonded state than in the unbonded state

II

Both ionic and covalent bonds fail to provide the participating atoms with a stable electron configuration

Ionic bonds are always stronger than covalent bonds

They break only when bombarded with electrons

BECAUSE

BECAUSE

73

I

The most important factor in determining the chemical properties of an element is the number of electrons in the outermost shell

II

The number of electrons in the outer shell determines the bonding characteristics of the element

Helium will have fewer dispersion forces between its atoms than the other noble gases

As the mass of nonpolar atoms and molecules increases, dispersion forces increase

BECAUSE

BECAUSE

74

Which of the following are the WEAKEST attractive force?

(A) Dipole-dipole forces(B) Coordinate covalent bonding(C) Covalent bonding(D) Polar covalent bonding(E) Ionic bonding

75

The complete loss of an electron of one atom to another atom with the consequent formation of electrostatic charges is referred to as

(A) A covalent bond(B) A polar covalent bond(C) An ionic bond(D) A coordinate covalent bond(E) A pi bond between p orbitals

76

Which of the following compounds would be predicted to have the highest melting point?

(A) CS2

(B) HI(C) H2S(D) H2O(E) MgO

77

Which compound is not paired with its correct name?

(A) FeCl2 / iron(II) chloride(B) K2O / potassium oxide(C) NO2 / nitrogen dioxide(D) PCl3 / potassium trichloride(E) NH4Cl / ammonium chloride

78

Which of the following statements about bonding is correct?

(A) Van der Waals forces exist between polar molecules

(B) Dipoles are the result of the equal sharing of electrons

(C) Cu(s) is a network solid(D) Hydrogen bonds exist between the molecules of

HCl(E) NaCl (aq) has attraction between the molecules

and the ions

79

Which kinds of bonding can be found in a sample of H2O (l)?

(A) Hydrogen bonds only(B) Nonpolar covalent bonds only(C) Ionic and nonpolar hydrogen bonds(D) Both polar covalent and hydrogen bonds(E) Metallic and ionic bonds

80

Which compound contains no ionic character?

(A) NH4Cl(B) CaO(C) K2O(D) Li2O(E) CO

81

The forces of attraction that exist between nonpolar molecules are called

(A) Van der Waals/ dispersion forces(B) Ionic bonds(C) Covalent bonds(D) Electrovalent bonds(E) Metallic bonds

82

When a salt dissolves in water, the water molecules are attracted by ions in solution. This attraction is called

(A) Atom-atom(B) Molecule-molecule(C) Molecule-ion(D) Ion-ion(E) Atom-ion

83

Which element is expected to have a “sea” of electrons?

(A) Hydrogen(B) Nitrogen(C) Cobalt(D) Chlorine(E) Oceanium

84

In which of the following liquids are the Van der Waals forces of attraction between the molecules weakest?

(A) Xe(B) Kr(C) Ar(D) Ne(E) He

85

Which molecule has both nonpolar intramolecular and nonpolar intermolecular bonds?

(A) CCl4

(B) CO(C) HF(D) HCl(E) F2

86

If two atoms that differ in electronegativity combine by chemical reaction and share electrons, the bond that joins them will be

(A) Metallic(B) Ionic(C) A hydrogen bond(D) Nonpolar covalent(E) Polar covalent

87

The reactivity and chemical behavior of an atom is governed by many factors. The most important factor is

(A) The number of protons in the nucleus(B) The number of neutrons in the nucleus(C) The number of protons and neutrons in the

nucleus(D) The ratio of protons and neutrons in the nucleus(E) The number of electrons in the valence shell