Deck 6: Ionic and Molecular Compounds

Question 1

What is the correct formula for the oxide ion?

A)O₂-
B)O-
C)O+
D)O₂+
E)O₃+

Answer 1

O₂-

Question 2

How many electrons will chlorine gain or lose when it forms an ion?

A)lose 1
B)gain 1
C)lose 7
D)gain 2
E)lose 3

Answer 2

gain 1

Question 3

In ionic compounds, ________ lose their valence electrons to form positively charged ________. (5,2)

A)metals; anions
B)nonmetals; cations
C)metals; polyatomic ions
D)nonmetals; anions
E)metals; cations

Answer 3

metals; cations

Question 4

How many valence electrons does carbon have?

A)one
B)two
C)three
D)four
E)five

Question 5

To form an ion, a sodium atom

A)gains one electron.
B)gains two electrons.
C)loses seven electrons.
D)loses one electron.
E)loses two electrons.

Question 6

The number of electrons in an ion with 20 protons and an ionic charge of 2+ is

A)24.
B)22.
C)20.
D)18.
E)16.

Question 7

The octet rule indicates that

A)all of the noble gases have eight total electrons.
B)all of the shells in an atom hold a maximum of 8 electrons.
C)all of the Group A elements have 8 valence electrons.
D)atoms lose, gain, or share valence electrons to have 8 valence electrons.
E)the noble gases react with other compounds to get 8 valence electrons.

Question 8

What is the symbol for the ion with 19 protons and 18 electrons?

A)F+
B)F-
C)Ar+
D)K-
E)K+

Question 9

What is the ionic charge of an ion with 13 protons and 10 electrons?

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

Question 10

Elements in group 2A(2) of the periodic table form ions with a charge of

A)1+.
B)1-.
C)2+.
D)3+.
E)0.

Question 11

The number of valence electrons found in an atom of a Group A element is equal to

A)its atomic number.
B)its mass number.
C)its group number.
D)eight.
E)eight minus the group number.

Question 12

How many valence electrons does nitrogen have?

A)one
B)two
C)three
D)four
E)five

Question 13

What is the formula of the nitride ion?

A)N₃-
B)NO₂-
C)NO₃^3-
D)NO₃^2-
E)NO₃-

Question 14

In an electron-dot structure of an element, the dots are used to represent

A)all of the electrons in the atom.
B)the valence electrons.
C)the electron arrangement.
D)only the electrons that will participate in bond formation.
E)the electrons that the element will gain when it forms a compound.

Question 15

How many electrons will lithium gain or lose when it forms an ion?

A)lose 1
B)gain 5
C)lose 2
D)lose 3
E)gain 1

Question 16

How many valence electrons are in the electron-dot structures for the elements in group 3A(13)?

A)1
B)2
C)3
D)4
E)6

Question 17

How many electrons will aluminum gain or lose when it forms an ion?

A)lose 1
B)gain 5
C)lose 2
D)lose 3
E)gain 1

Question 18

The ion of aluminum is

A)Al+.
B)Al₂+.
C)Al₃+.
D)Al₃-.
E)Al₂-.

Question 19

Valence electrons are electrons located

A)in the outermost energy level of an atom.
B)in the nucleus of an atom.
C)in the innermost energy level of an atom.
D)throughout the atom.
E) in the first three shells of an atom.

Question 20

An anion always

A)has a positive charge.
B)contains a group of two or more atoms with a positive charge.
C)contains a metal and a nonmetal.
D)forms covalent bonds.
E)has a negative charge.

Question 21

A group of covalently bonded atoms that has an overall electrical charge is called a(n)

A)ionic compound.
B)anion.
C)polyatomic ion.
D)cation.
E)molecule.

Question 22

What is the formula for aluminum nitrite?

A)Al₂NO₂
B)AlNO₃
C)Al(NO₂)₃
D)Al₂(NO₃)₃
E)Al₂(NO₂)₂

Question 23

The name of PbO₂ is

A)lead dioxide.
B)lead(II)oxide.
C)lead(IV)oxide.
D)plumbum oxide.
E)lead oxygen.

Question 24

What is the formula of a compound that contains Na⁺ and PO₄ ^3- ions?

A)Na₃PO₄
B)NaPO₄
C)Na₂PO₃
D)Na₃PO₃
E)Na₃P

Question 25

The compound MgCl₂ is named

A)magnesium chlorine.
B)magnesium dichloride.
C)magnesium(II)chloride.
D)magnesium chloride.
E)dimagnesium chloride.

Question 26

How many electrons will iodine gain or lose when it forms an ion?

A)lose 1
B)gain 5
C)lose 2
D)lose 3
E)gain 1

Question 27

The formula of copper(I) sulfide is

A)CuS.
B)Cu₂S.
C)Cu₂(SO₄)₃.
D)CuSO₄.
E)CuS₂.

Question 28

What is the correct formula for iron(III) sulfide?

A)Fe₂S₂
B)Fe₂S
C)FeS
D)FeS₂
E)Fe₂S₃

Question 29

An ionic compound

A)has a net positive charge.
B)has a net negative charge.
C)contains only cations.
D)contains only anions.
E)has a net charge of zero.

Question 30

Which of the following polyatomic ions has a positive charge?

A)hydroxide
B)sulfate
C)hydrogen carbonate
D)ammonium
E)nitrate

Question 31

The name of the HSO₄ - ion is

A)sulfate.
B)hydrogen sulfate.
C)sulfite.
D)hydrogen sulfite.
E)sulfide.

Question 32

Which of the following polyatomic ions has a 3- ionic charge?

A)hydroxide
B)nitrate
C)sulfate
D)phosphate
E)bicarbonate

Question 33

What is the correct formula for the iron(II) ion?

A)Fe⁺
B)Fe²⁺
C)Fe³⁺
D)Fe^2-
E)Fe^3-

Question 34

The name of Al₂(SO₄)₃ is

A)aluminum(III)sulfate.
B)dialuminum trisulfate.
C)dialuminum sulfate.
D)dialuminum trisulfide.
E)aluminum sulfate.

Question 35

The correct formula for the compound formed from Mg and S is

A)MgS.
B)MgS₂.
C)Mg₂S.
D)Mg₂S₂.
E)Mg₂S₃.

Question 36

Which one of the following elements forms two or more ions with different ionic charges?

A)K
B)F
C)Ca
D)O
E)Fe

Question 37

The correct formula for a compound formed from the elements Al and O is

A)AlO.
B)Al₂O.
C)Al₃O₂.
D)AlO₃.
E)Al₂O₃.

Question 38

The name of the Cu+ ion is

A)copper(II).
B)copper(I).
C)cobalt.
D)copper.
E)cuprum.

Question 39

Which one of the following compounds contains an ion with a 3+ charge?

A)KCl
B)Na₂O
C)FeCl₃
D)CuCl
E)MgCl₂

Question 40

Fe₂(SO₄)₃ is called

A)iron sulfate.
B)iron(II)sulfate.
C)iron(III)sulfate.
D)diiron trisulfate.
E)iron trisulfate.

Question 41

The correct name for the compound N₂O₃ is

A)nitrogen oxide.
B)nitrogen trioxide.
C)dinitride trioxide.
D)dinitrogen oxide.
E)dinitrogen trioxide.

Question 42

Which of the following compounds contains a polar covalent bond?

A)NaF
B)HCl
C)Br₂
D)MgO
E)O₂

Question 43

What is the formula of carbon tetraiodide?

A)CI
B)CI₄
C)C₄I
D)CI₃
E)C₂I₄

Question 44

Which of the following elements has the lowest electronegativity?

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

Question 45

The ability of an atom to attract the shared electrons in a covalent bond is its

A)electronegativity.
B)bonding ability.
C)polarity.
D)ionic character.
E)nonpolarity.

Question 46

Choose the best electron-dot structure for OCl₂ .

A)
B)
C)
D)
E)

Question 47

The types of compounds that use prefixes in their names are

A)ionic compounds.
B)ionic compounds involving transition metals.
C)polyatomic ions.
D)covalent compounds.
E)compounds that contain polyatomic ions.

Question 48

The correct name of the compound NCl₃ is

A)nitrogen chloride.
B)trinitrogen chloride.
C)nitrogen (III) chloride.
D)nickel chloride.
E)nitrogen trichloride.

Question 49

Double and triple bonds form because

A)the atoms involved have high electronegativities.
B)single covalent bonds do not give all of the atoms in the molecule eight valence electrons.
C)one of the atoms in the molecule has more than eight valence electrons.
D)the ions involved have charges larger than one.
E)there is at least one hydrogen atom involved in the bond.

Question 50

How many valence electrons are in the electron-dot structure of H₂O?

A)2
B)4
C)6
D)8
E)10

Question 51

Which of the following compounds contains an ionic bond?

A)NH₃
B)H₂O
C)CaO
D)H₂
E)CH₄

Question 52

How many valence electrons are in the electron-dot structure of CCl₄ ?

A)0
B)82
C)6
D)8
E)32

Question 53

Which of the following elements does NOT exist as a diatomic molecule?

A)hydrogen
B)nitrogen
C)chlorine
D)oxygen
E)carbon

Question 54

A(n) ________ is the smallest neutral unit of two or more atoms held together by a covalent bond.

A)ionic compound
B)nucleus
C)molecule
D)formula
E)unit

Question 55

The formula for a molecule formed from N and Cl would be

A)NCl.
B)NCl₂
C)NCl₃
D)N3Cl.
E)NCl5.

Question 56

In a molecule with covalent bonding

A)oppositely charged ions are held together by strong electrical attractions.
B)atoms of metals form bonds to atoms of nonmetals.
C)atoms of different metals form bonds.
D)atoms are held together by sharing electrons.
E)atoms of noble gases are held together by attractions between oppositely charged ions.

Question 57

In a covalently bonded molecule, the number of electrons that an atom shares with others is usually equal to the number of electrons

A)in the atom.
B)in its nucleus.
C)in all the atoms.
D)in its ion.
E)needed to give it a stable electron configuration.

Question 58

Which of the following substances contains a nonpolar covalent bond?

A)H₂O
B)NaCl
C)NH₃
D)MgF₂
E)N₂

Question 59

Choose the best electron-dot structure for CH₂Cl₂ .

A)
B)
C)
D)
E)

Question 60

How many lone pairs of electrons are in the electron-dot structure of H₂O?

A)0
B)1
C)2
D)3
E)4

Question 61

The VSEPR theory allows us to determine the most favorable

A)shape of a molecule.
B)charge on an ion.
C)color of a compound.
D)bond type for a molecule.
E)formula for a compound.

Question 62

Ionic bonding is expected in which of these compounds?

A)Cl₂
B)KF
C)OF₂
D)HF
E)H₂

Question 63

The strongest interactions between atoms of helium He are examples of

A)ionic bonds.
B)covalent bonds.
C)hydrogen bonds.
D)dipole-dipole interactions.
E)dispersion forces.

Question 64

The strongest interactions between molecules of hydrogen chloride are

A)ionic bonds.
B)covalent bonds.
C)hydrogen bonds.
D)dipole-dipole interactions.
E)dispersion forces.

Question 65

The bond in Cl₂ is a(n)

A)ionic bond.
B)nonpolar covalent bond.
C)metallic bond.
D)polar ionic bond.
E)no bond.

Question 66

The shape of the water molecule ( H₂O) is

A)linear.
B)tetrahedral.
C)pyramidal.
D)bent.
E)octagonal.

Question 67

The strongest interactions between molecules of iodine I₂ are examples of

A)ionic bonds.
B)covalent bonds.
C)hydrogen bonds.
D)dipole-dipole interactions.
E)dispersion forces.

Question 68

Hydrogen sulfide, H₂S, has a shape similar to

A)carbon dioxide.
B)carbon monoxide.
C)hydrogen chloride.
D)water.
E)carbon tetrachloride.

Question 69

The strongest interactions between molecules of hydrogen ( H₂) are

A)ionic bonds.
B)hydrogen bonds.
C)polar covalent.
D)dipole-dipole.
E)dispersion forces.

Question 70

The carbon tetrachloride molecule, CCl₄ , is

A)a polar molecule with polar bonds.
B)a nonpolar molecule with polar bonds.
C)a nonpolar molecule with nonpolar bonds.
D)a polar molecule with nonpolar bonds.
E)a polar molecule with ionic bonds.

Question 71

If the electronegativity difference between elements X and Y is 2.1, the bond between the elements X-Y is

A)ionic.
B)nonpolar ionic.
C)nonpolar covalent.
D)polar covalent.
E)impossible.

Question 72

The ammonia molecule ( NH₃) is

A)a polar molecule with polar bonds.
B)a nonpolar molecule with polar bonds.
C)a nonpolar molecule with nonpolar bonds.
D)a polar molecule with nonpolar bonds.
E)a polar molecule with ionic bonds.

Question 73

The strongest interactions in the compound sodium fluoride, NaF, are examples of

A)ionic bonds.
B)covalent bonds.
C)hydrogen bonds.
D)dipole-dipole interactions.
E)dispersion forces.

Question 74

The carbon tetrachloride molecule, CCl₄ , has the shape of a

A)tetrahedron.
B)square.
C)cube.
D)circle.
E)sphere.

Question 75

The shape of the carbon tetrachloride molecule is

A)linear.
B)square.
C)pyramidal.
D)tetrahedral.
E)octagonal.

Question 76

A polar covalent bond is found in which of these compounds?

A)H₂O
B)F₂
C)NaCl
D)H₂
E)N2

Question 77

The shape of the carbon dioxide (CO₂) is

A)linear.
B)square.
C)pyramidal.
D)hexagonal.
E)bent.

Question 78

The water molecule has a dipole with the negative portion

A)localized between the hydrogen atoms.
B)pointing toward the oxygen atom.
C)localized on one of the hydrogens.
D)pointing from the oxygen through the hydrogen atoms.
E)surrounding the molecule.

Question 79

The shape of the ammonia molecule ( NH₃) is

A)linear.
B)square.
C)pyramidal.
D)hexagonal.
E)octagonal.

Question 80

The strongest interactions between molecules of ammonia ( NH₃) are

A)ionic bonds.
B)hydrogen bonds.
C)polar covalent.
D)dipole-dipole.
E)dispersion forces.