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Worksheetschemistry final exam chapter 6
Total questions: 39
Worksheet time: 10hrs 45mins
1. Ionic bonds form as a result of the electrostatic attraction between
dipoles.
electrons.
ions.
nuclei.
2. A single covalent bond involves the sharing of
only one electron.
two electrons.
three electrons.
a variable number of electrons, which depends on the bonding atoms.
1. If two covalently bonded atoms move closer than a distance of the bond length, the potential energy of the atoms
becomes negative.
decreases.
increases.
remains constant.
2. The electrons involved in the formation of a covalent bond are a. transferred from one atom to another.
transferred from one atom to another.
found only in the s orbitals.
valence electrons.
in filled orbitals.
An ionic compound is not represented by a molecular formula because an ionic compound
does not contain bonds
can form crystalline solids
has no net charge.
lacks molecules.
Compared with the energies of neutral atoms that form the ions, a crystal lattice has
zero potential energy.
higher potential energy.
lower potential energy.
equal potential energy.
Chemical bonding in metals is
the same as ionic bonding.
the same as covalent bonding.
a combination of ionic and covalent bonding.
different from ionic or covalent bonding.
The valence electrons in a metallic bond
move freely throughout the network of metal atoms.
are shared equally between two metal atoms.
are shared equally between two metal atoms.
continuously move from one energy level to another.
Within a metal, the vacant orbitals in the atoms’ outer energy levels
repel valence electrons.
attract other metal atoms.
overlap
diffract light.
Which of the following properties is not explained by metallic bonding?
electrical conductivity
thermal conductivity
brittleness
ductility
Which of the following is the result of visible light absorbed by a metal?
Electrons move to higher energy levels and remain there.
Light at a frequency similar to the absorbed frequency is emitted.
Electrons fill the vacant orbitals.
Light is given off as a line spectrum.
Metals are malleable because when struck, one plane of metal atoms
can slide past another plane without breaking bonds.
cannot easily move out of the way.
moves in a way that maximizes the repulsive forces within the metal.
bonds to the plane directly beneath it.
Which is a measure of metallic bond strength?
electron affinity
electronegativity
specific heat capacity
enthalpy of vaporization
In general, as you move from right to left across any row of the periodic table, the strength of a metallic bond
increases.
decreases.
stays the same.
shows no trend.
Which of these is responsible for the good electrical conductivity of metals?
the arrangement of metal atoms in separate layers
the high density of metals atoms in the crystal lattice
the ability of electrons to move freely about the crystal structure
the fact that metal atoms contain many orbitals separated by very small energy
The arrangement of valence electrons in a metallic bond is best described as
fixed positions in a lattice
a sea of free-moving electrons
concentrated electron density around specific atoms
electron pairs existing in multiple bonds
The salts NaCl(s) and CaCl2(s)
are good conductors of electricity.
are positively charged.
are held together by ionic bonds.
Both (a) and (b)
Compared with solid ionic compounds, solid molecular compounds generally
have lower melting points.
are more brittle.
are harder.
conduct electricity as liquids.
Because strong attractive forces hold the layers in an ionic crystal in relatively fixed positions, ionic compounds
are hard.
are brittle.
are not electrical conductors as solids.
All of the above
In a crystal of sodium chloride, how many oppositely-charged ions does each Na+ and Clion have clustered around it?
1
2
4
6
The arrangement of ions within a crystal structure and the strengths of the attractions between them vary with the
sizes of the ions.
charges of the ions.
numbers of ions of different charges.
All of the above
The energy released when one mole of an ionic crystalline solid is formed from ions in the gas state is known as
thermal energy.
lattice energy.
ionization energy.
radiant energy.
Some ionic compounds do not dissolve in water because
the attractions between the water molecules and the ions are not as strong as the attractions between the ions.
they are less dense than water and float on the surface.
water is a covalent compound and covalent compounds cannot dissolve ionic compounds.
water molecules cannot fit in the spaces between the ions in the crystal lattice.
A charged group of covalently bonded atoms is known as a(n)
anion
polyatomic.
formula unit.
cation.
Bond energy is the energy
absorbed as a molecule forms
change as atoms get closer together.
required to break a chemical bond and form separate, neutral atoms.
of two covalently bonded atoms
Bond length between two bonded atoms is
twice the diameter of the molecular orbital.
the separation at which their potential energy is minimum.
the separation at which the motion of each atom stops.
the sum of the diameters of each of the two overlapping electron clouds.
Which compound most likely has the greatest bond energy?
HF; HF bond length = 92 pm
I2; II bond length = 266 pm
Cl2; ClCl bond length = 199 pm
HCl; HCl bond length = 127 pm
6. The Lewis structure of which of the following compounds does not follow the octet rule?
NH3
BF3
CCl4
H2O
In a double covalent bond,
one atom has more than eight valence electrons.
one atom loses a pair of electrons.
two atoms share eight valence electrons.
two atoms share two pairs of electrons.
How many double bonds are in the Lewis structure for hydrogen fluoride, HF?
none
one
two
three
To draw a Lewis structure, it is not necessary to know
the length of the bonds.
the types of atoms in the molecule.
the number of valence electrons for each atom.
the number of atoms in the molecule.
Use the table below to choose the pair of elements that will most likely have the least ionic character.
Na 0.9 O 3.5
Cl 3.0 H 2.1
Na and Cl
O and Cl
H and O
Na and O
Use the table below to choose the pair of elements that will most likely have the greatest ionic character.
K 0.8
N 3.0
Br 2.8
S 2.5
K and N
K and S
N and Br
S and Br
The measure of an atom’s ability to attract electrons is its
electronegativity
polarization.
ionization
electron affinity
Atoms that are bonded with an electronegativity difference of 0 to 0.3 are generally considered to be
negatively charged compounds.
nonpolar-covalent compounds.
polar-covalent compounds.
ionic compounds.
What is the apparent charge on the chlorine atom in the molecule HCl?
+1
-1
S+
S-
Atoms seldom exist as independent particles in nature because
as single particles, most atoms have low potential energy.
their electronegativity is much lower when they combine with other atoms.
atoms are more stable when they combine with other atoms.
neutral particles are rare.
When an atom completely gives up its valence electrons to another atom, they form a bond that is considered to be
purely ionic.
partially ionic.
polar-covalent.
nonpolar-covalent.
You can estimate the degree to which a bond between two atoms is ionic or covalent by calculating the
distance between the atoms’ nuclei
difference in the atoms’ electronegativities.
atoms’ atomic radii.
number of atoms in the compound.
