Max Mckenna
New member
1.
Covalent compounds have __________ structure, whereas ionic compounds have __________ structure.
A) an unorganized, a crystal lattice
B) a crystal lattice, a liquid
C) a crystal lattice, an unorganized
D) a liquid, a gas
2.
Ionic compounds are formed through __________, whereas covalent compounds are formed through electron __________.
A) proton sharing, sharing
B) electron exchange, sharing
C) proton exchange, sharing
D) electron sharing, exchange
3.
Ionic bonds are usually made between metals and nonmetals, whereas covalent bonds are
A) usually made by two metals.
B) usually formed by two nonmetals.
C) usually not formed by two nonmetals.
D) formed between metals and nonmetals.
4.
When atoms form a polar covalent bond, what happens to their charges?
A) The atom with the least attraction for electrons takes on a negative charge.
B) The atom with the most attraction for electrons takes on a partial negative charge.
C) The atom with the most attraction for electrons takes on a partial positive charge.
D) The charges on atoms in a polar covalent bond are negative.
5.
In a polar covalent bond,
A) electrons are shared equally between atoms.
B) a cation is bonded to an anion.
C) electrons are transferred between atoms.
D) electrons are not shared equally between atoms.
6.
If the difference in electronegativity values of two elements is around 0.4, which bond is likely to form?
A) A polar covalent bond
B) A nonpolar covalent bond
C) An ionic bond
D) A molecular orbital bond
7.
If the difference in electronegativity values of two elements is around 3.0, which bond is likely to form?
A) A polar covalent bond
B) A nonpolar covalent bond
C) An ionic bond
D) A molecular orbital bond
8.
If the difference in electronegativity values of two elements is around 1.2, which bond is likely to form?
A) A polar covalent bond
B) A nonpolar covalent bond
C) An ionic bond
D) A molecular orbital bond
9.
At room temperature, ionic compounds are typically solids, whereas covalent compounds are
A) gases.
B) liquids.
C) hydrogen.
D) solids, liquids, or gases.
10.
Ionic compounds have __________ melting points and covalent compounds have __________ melting points.
A) low, high
B) high, high
C) low, low
D) high, low
11.
If two hydrogen atoms share their electrons and form a covalent bond,
A) they will have a negative charge.
B) they will have a positive charge.
C) one of the atoms will become a helium atom.
D) they will achieve a stable electron configuration.
12.
Why does a covalent compound have a low melting point?
A) A covalent compound has strong bonds.
B) A covalent compound contains no bonds.
C) The structure of a covalent compound is unorganized.
D) A covalent compound is brittle.
13.
A covalent compound is
A) an effective conductor of electricity.
B) a poor conductor of electricity.
C) brittle when struck with a hammer.
D) organized with a clearly defined structure.
14.
When struck with a hammer, a covalent compound
A) will not shatter into pieces.
B) will shatter into pieces.
C) becomes a polar covalent compound.
D) becomes an ionic compound.
15.
Which of these exists as a diatomic molecule in nature?
A) Fe2
B) Hg2
C) Cl2
D) As2
16.
Which of these does NOT exist as a diatomic molecule in nature?
A) Br2
B) Au2
C) I2
D) F2
17.
To indicate resonance, a __________ is placed between a molecule’s resonance structures.
A) single-headed arrow
B) series of three raised dots
C) long dash
D) double-headed arrow
18.
The correct Lewis structure for the oxygen atom has
A) one pair of valence electrons and a single valence electron.
B) two pairs of valence electrons and a single valence electron.
C) two pairs of valence electrons and two single valence electrons.
D) three pairs of valence electrons.
19.
The correct Lewis structure for a group 18 atom has
A) one pair of valence electrons and a single valence electron.
B) two pairs of valence electrons and a single valence electron.
C) three pairs of valence electrons and a single valence electron.
D) four pairs of valence electrons.
20.
The correct Lewis structure for a molecule of the compound C2H2 contains
A) three single bonds.
B) two double bonds.
C) three double bonds.
D) one triple bond.
Covalent compounds have __________ structure, whereas ionic compounds have __________ structure.
A) an unorganized, a crystal lattice
B) a crystal lattice, a liquid
C) a crystal lattice, an unorganized
D) a liquid, a gas
2.
Ionic compounds are formed through __________, whereas covalent compounds are formed through electron __________.
A) proton sharing, sharing
B) electron exchange, sharing
C) proton exchange, sharing
D) electron sharing, exchange
3.
Ionic bonds are usually made between metals and nonmetals, whereas covalent bonds are
A) usually made by two metals.
B) usually formed by two nonmetals.
C) usually not formed by two nonmetals.
D) formed between metals and nonmetals.
4.
When atoms form a polar covalent bond, what happens to their charges?
A) The atom with the least attraction for electrons takes on a negative charge.
B) The atom with the most attraction for electrons takes on a partial negative charge.
C) The atom with the most attraction for electrons takes on a partial positive charge.
D) The charges on atoms in a polar covalent bond are negative.
5.
In a polar covalent bond,
A) electrons are shared equally between atoms.
B) a cation is bonded to an anion.
C) electrons are transferred between atoms.
D) electrons are not shared equally between atoms.
6.
If the difference in electronegativity values of two elements is around 0.4, which bond is likely to form?
A) A polar covalent bond
B) A nonpolar covalent bond
C) An ionic bond
D) A molecular orbital bond
7.
If the difference in electronegativity values of two elements is around 3.0, which bond is likely to form?
A) A polar covalent bond
B) A nonpolar covalent bond
C) An ionic bond
D) A molecular orbital bond
8.
If the difference in electronegativity values of two elements is around 1.2, which bond is likely to form?
A) A polar covalent bond
B) A nonpolar covalent bond
C) An ionic bond
D) A molecular orbital bond
9.
At room temperature, ionic compounds are typically solids, whereas covalent compounds are
A) gases.
B) liquids.
C) hydrogen.
D) solids, liquids, or gases.
10.
Ionic compounds have __________ melting points and covalent compounds have __________ melting points.
A) low, high
B) high, high
C) low, low
D) high, low
11.
If two hydrogen atoms share their electrons and form a covalent bond,
A) they will have a negative charge.
B) they will have a positive charge.
C) one of the atoms will become a helium atom.
D) they will achieve a stable electron configuration.
12.
Why does a covalent compound have a low melting point?
A) A covalent compound has strong bonds.
B) A covalent compound contains no bonds.
C) The structure of a covalent compound is unorganized.
D) A covalent compound is brittle.
13.
A covalent compound is
A) an effective conductor of electricity.
B) a poor conductor of electricity.
C) brittle when struck with a hammer.
D) organized with a clearly defined structure.
14.
When struck with a hammer, a covalent compound
A) will not shatter into pieces.
B) will shatter into pieces.
C) becomes a polar covalent compound.
D) becomes an ionic compound.
15.
Which of these exists as a diatomic molecule in nature?
A) Fe2
B) Hg2
C) Cl2
D) As2
16.
Which of these does NOT exist as a diatomic molecule in nature?
A) Br2
B) Au2
C) I2
D) F2
17.
To indicate resonance, a __________ is placed between a molecule’s resonance structures.
A) single-headed arrow
B) series of three raised dots
C) long dash
D) double-headed arrow
18.
The correct Lewis structure for the oxygen atom has
A) one pair of valence electrons and a single valence electron.
B) two pairs of valence electrons and a single valence electron.
C) two pairs of valence electrons and two single valence electrons.
D) three pairs of valence electrons.
19.
The correct Lewis structure for a group 18 atom has
A) one pair of valence electrons and a single valence electron.
B) two pairs of valence electrons and a single valence electron.
C) three pairs of valence electrons and a single valence electron.
D) four pairs of valence electrons.
20.
The correct Lewis structure for a molecule of the compound C2H2 contains
A) three single bonds.
B) two double bonds.
C) three double bonds.
D) one triple bond.