WorksheetsHonors Unit 4 Bonding and Molecular Geometry
Total questions: 100
Worksheet time: 50mins
Name
Class
Date
1.
What type of bond involves the transfer of electrons from a metal to a nonmetal?
a)
Covalent bond
b)
Metallic bond
c)
Hydrogen bond
d)
Ionic bond
e)
Coordinate bond
2.
Which of the following is NOT a property of ionic compounds?
a)
High melting points
b)
Conductivity in molten form
c)
Form discrete molecules
d)
Brittleness
e)
Crystal lattice formation
3.
What is the primary type of bonding in a sample of copper metal?
a)
Ionic bonding
b)
Covalent bonding
c)
Hydrogen bonding
d)
Metallic bonding
e)
Coordinate bonding
4.
What explains why metals are malleable and conduct electricity well?
a)
Strong ionic attractions
b)
Shared electron pairs
c)
Delocalized electrons
d)
Low electronegativity
e)
Covalent crystal structures
5.
In covalent bonding, electrons are:
a)
Transferred from one atom to another
b)
Shared between nonmetals
c)
Delocalized among ions
d)
Trapped in crystal lattices
e)
Moved into d-orbitals
6.
Select all that are properties of metallic substances.
a)
Ductile
b)
Shiny
c)
Poor conductor
d)
High melting point
e)
Form discrete molecules
7.
Which bond type is characterized by a 'sea of electrons'?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Hydrogen
e)
Polar
8.
Which element combination is most likely to form an ionic bond?
a)
Oxygen and chlorine
b)
Sodium and fluorine
c)
Carbon and hydrogen
d)
Nitrogen and oxygen
e)
Chlorine and bromine
9.
Covalent compounds tend to have:
a)
High melting points and high conductivity
b)
Crystal lattices and ionic bonds
c)
Low melting points and no conductivity
d)
Free-flowing electrons
e)
Strong ion-dipole forces
10.
In metallic bonding, the strength of the bond increases with:
a)
Atomic radius
b)
Number of protons
c)
Electron affinity
d)
Number of valence electrons
e)
Atomic mass
11.
The electrostatic force between oppositely charged ions is responsible for which bond?
a)
Covalent
b)
Hydrogen
c)
Ionic
d)
Metallic
e)
Dipole-dipole
12.
Fill in the blank: Ionic bonding occurs between a ______ and a ______.
(a)
13.
Which of the following is a good example of a covalently bonded substance?
a)
NaCl
b)
CaO
c)
CH₄
d)
Fe
e)
KBr
14.
What is the name for the 3D structure formed by ions in an ionic compound?
a)
Molecular orbital
b)
Covalent grid
c)
Crystal lattice
d)
Electron cloud
e)
Dipole structure
15.
Which principle explains why ionic bonds form between metals and nonmetals?
a)
Conservation of mass
b)
Electron shielding
c)
Octet rule
d)
Le Chatelier’s principle
e)
Bond polarity
16.
What is a crystal lattice?
a)
A disordered structure of atoms
b)
A molecule of metals
c)
A 3D arrangement of ions
d)
A group of shared electrons
e)
A cloud of delocalized electrons
17.
Ionic compounds are generally brittle because:
a)
They have strong dipole interactions
b)
Their ions repel when misaligned
c)
They lack bonding electrons
d)
They are nonpolar
e)
They contain lone pairs
18.
Which of the following pairs would produce the strongest ionic bond?
a)
Na⁺ and Cl⁻
b)
K⁺ and Br⁻
c)
Mg²⁺ and O²⁻
d)
Li⁺ and F⁻
e)
Ca²⁺ and I⁻
19.
What is lattice energy?
a)
Energy needed to break covalent bonds
b)
Energy required to melt a metal
c)
Energy released when gaseous ions form a solid
d)
Energy absorbed during bond formation
e)
Energy lost in reactions
20.
According to Coulomb’s Law, the force of attraction between ions increases with:
a)
Lower charges and larger radii
b)
Higher charges and smaller radii
c)
More valence electrons
d)
High electronegativity
e)
Greater molar mass
21.
Which compound would have the highest lattice energy?
a)
NaCl
b)
LiF
c)
MgO
d)
KBr
e)
CaCl₂
22.
Which of the following properties is NOT typical of ionic compounds?
a)
Hardness
b)
Electrical conductivity in solid state
c)
Solubility in water
d)
High melting point
e)
Formation of crystals
23.
In NaCl, what happens to the sodium atom during bond formation?
a)
It shares electrons with Cl
b)
It gains an electron
c)
It becomes a negatively charged ion
d)
It loses an electron
e)
It forms a covalent bond
24.
Which phrase best describes the behavior of ions in a salt crystal?
a)
Move freely like electrons
b)
Are bonded by shared electron pairs
c)
Form overlapping molecular orbitals
d)
Occupy fixed positions in a lattice
e)
Vibrate in covalent networks
25.
Write the formula for the compound formed by magnesium and chlorine.
(a)
26.
What does the strength of the electrostatic force depend on, according to Coulomb’s Law?
a)
Valence electrons and electronegativity
b)
Atomic mass and molar volume
c)
Ionic charge and distance
d)
Bond length and hybridization
e)
Boiling point and polarity
27.
Choose all that apply to ionic compounds.
a)
Conduct electricity in water
b)
Low melting points
c)
Form formula units
d)
Contain metal and nonmetal
e)
Form discrete molecules
28.
What happens to ionic conductivity when an ionic compound is dissolved in water?
a)
Increases
b)
Decreases
c)
Stays the same
d)
Becomes zero
e)
Depends on polarity
29.
Covalent bonding occurs primarily between which types of elements?
a)
Metals only
b)
Nonmetals only
c)
Metals and nonmetals
d)
Transition metals
e)
Noble gases
30.
Which of the following is a characteristic of a covalent compound?
a)
Conductive when solid
b)
Forms ions in water
c)
Discrete molecules
d)
High boiling point
e)
Shiny surface
31.
A single covalent bond involves how many shared electrons?
a)
1
b)
2
c)
3
d)
4
e)
6
32.
What is a coordinate covalent bond?
a)
Electrons transferred from metal to nonmetal
b)
Delocalized electron sharing in metals
c)
A bond where both electrons come from one atom
d)
Unequal sharing of electrons
e)
A bond formed between ions
33.
Which of the following molecules contains a double bond?
a)
CH₄
b)
CO₂
c)
NH₃
d)
H₂O
e)
NaCl
34.
How many valence electrons are in a water molecule?
a)
4
b)
6
c)
8
d)
10
e)
12
35.
Choose all valid steps in drawing a Lewis structure.
a)
Count total valence electrons
b)
Form bonds between all atoms
c)
Place central atom with lowest electronegativity
d)
Maximize lone pairs on metals
e)
Use multiple bonds if needed
36.
Which is the correct Lewis structure for CO₂?
a)
O–C–O
b)
O=C–O
c)
O=C=O
d)
C≡O–O
e)
C–O–O
37.
What causes a bond to be polar?
a)
Bond angle greater than 109.5°
b)
Same electronegativity
c)
Unequal sharing of electrons
d)
Excess lone pairs
e)
High melting point
38.
Which element has the highest electronegativity?
a)
Oxygen
b)
Nitrogen
c)
Chlorine
d)
Fluorine
e)
Carbon
39.
What is the molecular shape of NH₃?
a)
Tetrahedral
b)
Linear
c)
Trigonal pyramidal
d)
Bent
e)
Octahedral
40.
Which of the following molecules is nonpolar?
a)
H₂O
b)
CH₄
c)
NH₃
d)
HF
e)
SO₂
41.
Draw the Lewis structure for CH₄.
(a)
42.
Which of the following correctly matches bond type with shared pairs?
a)
Single bond – 4 electrons
b)
Double bond – 3 electrons
c)
Triple bond – 2 electrons
d)
Triple bond – 3 pairs
e)
Single bond – 3 pairs
43.
What does VSEPR stand for?
a)
Valence Shell Electron Pair Repulsion
b)
Very Simple Electron Pairing Rule
c)
Valence State Electron Position Rule
d)
Variable Shell Electron Potential Repulsion
e)
Valence Spin Energy Pair Rule
44.
What determines molecular geometry according to VSEPR theory?
a)
Type of atoms only
b)
Size of the central atom
c)
Number of electron domains
d)
Number of protons
e)
Bond energy
45.
Which shape does CH₄ exhibit?
a)
Linear
b)
Trigonal planar
c)
Bent
d)
Tetrahedral
e)
Trigonal bipyramidal
46.
What is the bond angle in a trigonal planar molecule?
a)
180°
b)
120°
c)
109.5°
d)
90°
e)
104.5°
47.
Which of the following molecules has a bent shape?
a)
BF₃
b)
CO₂
c)
H₂O
d)
CH₄
e)
CCl₄
48.
What causes molecular shapes like 'bent' or 'trigonal pyramidal'?
a)
Presence of metal atoms
b)
Polarity of bonds
c)
Presence of lone pairs
d)
Type of elements involved
e)
Ionization energy
49.
Choose all examples of linear geometry.
a)
CO₂
b)
H₂O
c)
HF
d)
CH₄
e)
BeCl₂
50.
Which of the following has a trigonal planar shape?
a)
BF₃
b)
NH₃
c)
H₂O
d)
CCl₄
e)
N₂
51.
Predict the molecular geometry for SF₄.
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Square planar
d)
See-saw
e)
Octahedral
52.
Which bond angle is closest to that found in a tetrahedral molecule?
a)
120°
b)
180°
c)
104.5°
d)
109.5°
e)
90°
53.
How many electron domains are around the central atom in PCl₅?
a)
3
b)
4
c)
5
d)
6
e)
2
54.
Which of these shapes results from a molecule with four domains and one lone pair?
a)
Bent
b)
Tetrahedral
c)
Trigonal pyramidal
d)
Trigonal planar
e)
Octahedral
55.
What is the shape of XeF₄?
a)
Square planar
b)
See-saw
c)
Tetrahedral
d)
Linear
e)
Octahedral
56.
Name the molecular geometry of H₂O.
(a)
57.
What does electronegativity describe?
a)
Ability to form ions
b)
Energy to remove an electron
c)
Attraction for shared electrons
d)
Number of valence electrons
e)
Mass of an atom
58.
Which atom has the greatest electronegativity?
a)
Oxygen
b)
Chlorine
c)
Nitrogen
d)
Carbon
e)
Fluorine
59.
Which bond is most polar based on electronegativity difference?
a)
C–H
b)
O–H
c)
Cl–Cl
d)
N–O
e)
C–C
60.
How does bond polarity relate to molecular polarity?
a)
They are unrelated
b)
Only symmetrical bonds are polar
c)
Polarity of bonds contributes to net dipole
d)
Molecular polarity determines bond type
e)
Polarity is irrelevant in molecules
61.
In CO₂, why is the molecule nonpolar?
a)
All atoms are the same
b)
Oxygen is less electronegative
c)
It has polar bonds but is linear and symmetric
d)
It has lone pairs
e)
It contains only nonmetals
62.
What is the dipole moment?
a)
Bond angle in a molecule
b)
Number of lone pairs
c)
Energy released when bonds form
d)
Measure of molecular polarity
e)
Ionization potential
63.
Which molecule is polar due to its asymmetrical shape?
a)
CH₄
b)
CO₂
c)
CCl₄
d)
NH₃
e)
CF₄
64.
Choose all that describe polar molecules.
a)
Have net dipole moments
b)
Symmetrical shape
c)
Unequal electron sharing
d)
Canceling dipoles
e)
Asymmetrical distribution of charge
65.
Fill in the blank: Bond polarity arises from a difference in (a) .
66.
Which best explains why HF is a polar molecule?
a)
Both atoms are metals
b)
It has symmetrical shape
c)
Fluorine is more electronegative than hydrogen
d)
Bond is nonpolar
e)
Both atoms share electrons equally
67.
How can you determine if a molecule is polar?
a)
Count atomic mass
b)
Check for metal atoms
c)
Analyze bond polarity and shape
d)
See if it’s a gas
e)
Look at melting point
68.
Which molecule is nonpolar despite having polar bonds?
a)
NH₃
b)
H₂O
c)
CO₂
d)
HF
e)
CH₃Cl
69.
Which vector direction would the dipole arrow point in an H–F bond?
a)
Toward H
b)
Away from F
c)
Toward F
d)
Toward center
e)
No direction
70.
The ΔEN between two atoms is 1.2. What type of bond is this?
a)
Nonpolar covalent
b)
Polar covalent
c)
Ionic
d)
Metallic
e)
Dipole-dipole
71.
What are intermolecular forces (IMFs)?
a)
Forces within molecules
b)
Bonds between atoms
c)
Attractions between molecules
d)
Forces causing radioactivity
e)
Electron pair repulsions
72.
Which is the strongest type of IMF?
a)
London dispersion
b)
Hydrogen bonding
c)
Dipole-dipole
d)
Ion-dipole
e)
Van der Waals
73.
Which IMF is present in all molecules?
a)
Hydrogen bonding
b)
Dipole-dipole
c)
London dispersion
d)
Ion-dipole
e)
Ionic bonding
74.
What condition is necessary for hydrogen bonding?
a)
H bonded to a metal
b)
H bonded to O, N, or F
c)
H bonded to any nonmetal
d)
H in a polar molecule
e)
Presence of lone pairs
75.
Which compound exhibits hydrogen bonding?
a)
CH₄
b)
HCl
c)
H₂O
d)
CO₂
e)
NaCl
76.
Choose all factors that increase boiling point.
a)
Stronger IMFs
b)
Larger molecular mass
c)
More polar bonds
d)
Lower molar mass
e)
Symmetrical shape
77.
What IMF primarily accounts for CO₂’s low boiling point?
a)
Hydrogen bonding
b)
Ion-dipole
c)
Dipole-dipole
d)
London dispersion
e)
Metallic bonding
78.
Why does ethanol evaporate faster than water?
a)
Higher molar mass
b)
Weaker hydrogen bonding
c)
More polarity
d)
Stronger ion-dipole forces
e)
Low density
79.
How does polarity affect solubility?
a)
Nonpolar dissolves polar
b)
Polarity has no effect
c)
Polar dissolves polar
d)
Polar dissolves nonpolar
e)
Nonpolar dissolves in water
80.
Fill in the blank: IMFs become (a) as molecular size increases.
81.
Which IMF is dominant in NaCl dissolved in water?
a)
London dispersion
b)
Hydrogen bonding
c)
Dipole-dipole
d)
Ion-dipole
e)
Metallic bonding
82.
What IMF is present in CHCl₃?
a)
London dispersion and dipole-dipole
b)
Only hydrogen bonding
c)
Only ionic bonding
d)
Only dipole-dipole
e)
None
83.
Which property increases with stronger IMFs?
a)
Volatility
b)
Evaporation rate
c)
Surface tension
d)
Gas pressure
e)
Molecular size
84.
Identify all molecules likely to show hydrogen bonding.
a)
HF
b)
NH₃
c)
CH₄
d)
CO₂
e)
H₂O
85.
What explains why water forms droplets on surfaces?
a)
High electronegativity
b)
Metallic bonding
c)
Ion-dipole forces
d)
High surface tension from hydrogen bonds
e)
Capillary action
86.
What is the correct name for CO₂?
a)
Carbon monoxide
b)
Carbon dioxide
c)
Dicarbon monoxide
d)
Monocarbon dioxide
e)
Carbon oxide
87.
What is the correct name for PCl₃?
a)
Phosphorus trichloride
b)
Phosphorus chloride
c)
Triphosphorus chloride
d)
Chlorine phosphorus
e)
Phosphorus(III) chloride
88.
What prefix is used for four atoms in molecular naming?
a)
Tri-
b)
Penta-
c)
Tetra-
d)
Quad-
e)
Octa-
89.
Which of the following is a correct name-formula pair?
a)
Sulfur hexachloride – SCl₆
b)
Carbon tetrachloride – CCl₂
c)
Dinitrogen trioxide – NO₂
d)
Nitrogen monoxide – N₂O
e)
Phosphorus pentachloride – PCl₃
90.
Which of the following molecules is correctly matched with its geometry?
a)
CH₄ – Linear
b)
NH₃ – Trigonal pyramidal
c)
CO₂ – Bent
d)
H₂O – Tetrahedral
e)
BF₃ – Tetrahedral
91.
Choose all shapes with bond angles less than 109.5°.
a)
Bent (H₂O)
b)
Trigonal planar
c)
Tetrahedral
d)
Trigonal pyramidal
e)
See-saw
92.
What is the molecular shape of SF₆?
a)
Octahedral
b)
Tetrahedral
c)
Square planar
d)
Trigonal bipyramidal
e)
Bent
93.
How many atoms are present in one molecule of N₂O₅?
a)
5
b)
6
c)
7
d)
2
e)
3
94.
Write the name for the compound SF₄.
(a)
95.
Identify the geometry of ClF₃.
a)
Square planar
b)
Trigonal pyramidal
c)
T-shaped
d)
Bent
e)
Linear
96.
Which of the following molecules exhibits an expanded octet?
a)
CH₄
b)
CO₂
c)
PCl₅
d)
NH₃
e)
H₂O
97.
Determine the shape of XeF₂.
a)
Bent
b)
T-shaped
c)
Linear
d)
See-saw
e)
Octahedral
98.
Which real molecule exhibits hydrogen bonding, bent shape, and high boiling point?
a)
CO₂
b)
HF
c)
NH₃
d)
H₂O
e)
CH₄
99.
Name the molecular compound N₂O₅.
a)
Dinitrogen pentoxide
b)
Nitrogen dioxide
c)
Nitrogen monoxide
d)
Pentanitrogen dioxide
e)
Nitrate oxide
100.
Which shape best describes the arrangement of atoms in BrF₅?
a)
Tetrahedral
b)
Square pyramidal
c)
Trigonal planar
d)
Octahedral
e)
Square planar
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