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Worksheetspt2 -chem
Total questions: 89
Worksheet time: 52mins
Which IMF is present in ALL molecules?
Dipole-dipole
Hydrogen bonds
London dispersion forces
Ionic bonds
Which molecule has only LDF?
H₂O
NH₃
CH₄
HF
Which molecule has hydrogen bonding?
CH₄
HCl
H₂O
H₂S
Which IMF is strongest?
LDF
Dipole-dipole
Hydrogen bonds
They're all equal
Why does H₂O have a higher boiling point than H₂S?
Why can you smell gasoline but not water?
Gasoline has weak IMFs, so molecules escape easily
Water has strong IMFs, so molecules don't escape
Gasoline is more volatile
All of the above
Which has stronger LDF: F₂ or I₂?
F₂ (more electronegative)
I₂ (more electrons)
They're equal
Can't determine
Why does I₂ exist as a solid at room temperature while F₂ is a gas?
I₂ has stronger LDF (more electrons)
F₂ is more reactive
I₂ has ionic bonds
F₂ has hydrogen bonds
Which compound would have the highest boiling point?
A) CH₄ (LDF only)
B) HCl (LDF + dipole-dipole)
C) H₂O (LDF + dipole-dipole + H-bonds)
D) CO₂ (LDF only)
Which would be most volatile?
H₂O
CH₄
Which would most likely be a solid at room temperature?
F₂
Cl₂
Br₂
I₂
Which would dissolve in water?
NaCl (ionic)
CH₄ (nonpolar)
CCl₄ (nonpolar)
Both A and B
Why does NaCl dissolve in water but CCl₄ doesn't?
NaCl is ionic, CCl₄ is covalent
Water's polarity breaks ionic lattice
CCl₄ only has weak LDF with water (insufficient)
All of the above
Which would conduct electricity when dissolved in water?
NaCl
C₆H₁₂O₆ (glucose)
CH₄
All of the above
Why does tap water conduct but distilled water doesn't?
Tap water has dissolved ions
Distilled water has no ions
Ions can carry electric current
All of the above
Which trend is correct for the halogens (F₂, Cl₂, Br₂, I₂)?
Boiling point decreases down the group
State changes from solid to gas down the group
Compare H2O and H2S. Why does H2O have a higher boiling point?
H2O has more atoms
H2O has hydrogen bonds, H2S has only dipole-dipole
H2O is smaller
H2S has stronger bonds
Compare CO2 and SO2. Why is CO2 nonpolar but SO2 is polar?
CO2 has no lone pairs (symmetric), SO2 has lone pair (asymmetric)
CO2 has double bonds
SO2 has more atoms
Carbon is less electronegative
Compare CH4 and CH3OH. Which has stronger IMFs?
CH4 (more atoms)
CH3OH (has H-bonds and polarity)
They're equal
Can't determine
Which correctly explains why ionic compounds conduct when dissolved?
Ions are free to move
Water breaks the lattice
Water's polarity causes dissociation
All of the above
Which correctly explains why covalent compounds don't conduct?
They have no ions
They form discrete molecules
Electrons are shared, not transferred
All of the above
How does water dissolve an ionic compound?
Water forms covalent bonds with ions
Water's polarity attracts ions, breaking the lattice
Water creates new ionic bonds
Water breaks covalent bonds
Why do lone pairs compress bond angles?
They're smaller than bonding pairs
They have higher electron density, stronger repulsion
They attract bonding pairs
They're closer to the nucleus
Why do electron domains repel each other?
They're all positive
They're all negative (like charges repel)
They have no charge
They attract each other
Why does LDF exist in nonpolar molecules?
Electrons are constantly moving, creating temporary dipoles
Nonpolar molecules have permanent dipoles
Nonpolar molecules form ionic bonds
It doesn't exist in nonpolar molecules
Why are hydrogen bonds stronger than dipole-dipole forces?
A) Hydrogen is very small
B) F, O, N are very electronegative, creating strong dipoles
C) Close approach is possible
D) All of the above
Q14.6 More electrons = stronger LDF because:
There are more temporary dipoles formed.
Electrons repel each other more strongly.
Atoms become more stable.
Molecules become polar.
Which statement is correct regarding electron cloud polarizability?
More electrons = larger electron cloud = more polarizable
More electrons = more permanent dipoles
More electrons = stronger bonds
More electrons = ionic character
Why do symmetric molecules with polar bonds become nonpolar?
The bonds aren't actually polar
Dipole moments cancel out due to symmetry
Symmetry makes bonds weaker
Symmetric molecules can't be polar
Why do transition metals need Roman numerals in names?
They can form multiple charges
The formula doesn't indicate which charge
Roman numeral specifies the exact charge
All of the above
Which element follows the duet rule instead of octet?
Be
B
H
Li
Which metal has a fixed charge and doesn't need a Roman numeral?
Fe
Cu
Zn
Ni
What is the charge on Hg₂²⁺?
(a)
Which prefix is never used on the first element in covalent naming?
di-
tri-
mono-
tetra-
Why is CO named "carbon monoxide" not "carbon monooxide"?
Vowel dropping rule
Carbon doesn't need a prefix
It's arbitrary
Oxygen always gets "mono-"
Which polyatomic ion acts like a metal in naming?
NO3-
SO4 2-
NH4+
OH-
What is the difference between "bi-" and "di-" prefixes?
bi- = hydrogen added, di- = two atoms
They're the same
bi- = two atoms, di- = hydrogen added
bi- is for acids, di- is for covalent
Which geometry exception applies to diatomic molecules?
They're always bent
They're always linear (2 atoms)
They have no geometry
They're always trigonal planar
Q15.9 Elements that can have expanded octets (more than 8 electrons) include:
Elements in period 3 and beyond
Only hydrogen and helium
Only alkali metals
Elements in period 2
How many electrons does Be typically have in its valence shell when bonded?
2
4
6
8
How many electrons does B typically have in its valence shell when bonded?
3
4
6
8
Which noble gas can bond in rare cases?
He
Ne
Ar
Xe
What is the name of HBrO₃?
Hydrobromic acid
Bromic acid
Perbromic acid
Hypobromous acid
What is the name of HIO?
(a)
What is the name of H3PO3?
Phosphoric acid
Phosphorous acid
Hydrophosphoric acid
Hydrogen phosphite
What is the name of C2O42− ?
Carbonate
Oxalate
Acetate
Oxalate ion
What is the name of MnO4− ?
Manganate
Permanganate
Manganese oxide
Manganese(VII) oxide
What is the name of O22− ?
Oxide
Peroxide
Superoxide
Dioxide
What is the name of SnCl4?
Tin chloride
Tin(II) chloride
Tin(IV) chloride
What is the name of PbO₂?
Lead oxide
Lead(II) oxide
Lead(IV) oxide
Plumbic oxide
What does the HONC rule state about typical bond numbers?
H=1, O=2, N=3, C=4 bonds
H=2, O=2, N=3, C=4 bonds
H=1, O=1, N=2, C=3 bonds
It's always true, never exceptions
In a Lewis structure for an ion, what should you use?
Parentheses
Brackets
Curly braces
Nothing special
When drawing Lewis structures, polyatomic ions should be:
Separated into individual atoms
Kept together as a unit
Drawn separately
Ignored
What is the "point of maximum attraction" in covalent bonding?
Where atoms are closest
Optimal balance between attraction and repulsion
Where electrons are shared equally
Where the bond is strongest
What does bond dissociation energy represent?
Energy released when bond forms
Energy required to break a bond
Strength of the bond
Both B and C
Which bond type is shortest and strongest?
Single bond
Double bond
Triple bond
They're all equal
In resonance structures, electrons are:
Localized to specific bonds
Delocalized (can move)
Always in the same place
Not involved
Why does delocalization increase stability?
Electrons are more spread out
Lower energy state
More stable electron arrangement
All of the above
What does δ⁺ represent?
Full positive charge
Partial positive charge
Negative charge
No charge
What is electron density?
Number of electrons
Concentration of electrons in a region
Charge of electrons
Speed of electrons
Which property is NOT directly related to IMF strength?
A) Boiling point
B) Surface tension
C) Viscosity
D) Atomic number
What is surface tension?
Force at surface of liquid
Molecules at surface pulled inward by IMFs
Creates "skin" on surface
All of the above
What is viscosity?
Thickness of a liquid
Resistance to flow
Related to IMF strength
All of the above
What is capillary action?
Water climbing up narrow tubes
Due to adhesion and cohesion
Related to hydrogen bonding
All of the above
Which correctly describes the relationship between polarity and reactivity?
More polar = more reactive
Less polar = less reactive
Polarity creates distinct positive/negative ends that can interact
All of the above
Using the crisscross method for Mg²⁺ and Cl⁻, what is the formula?
MgCl
MgCl₂
Mg₂Cl
MgCl₃
Using the crisscross method for Al³⁺ and O²⁻, what is the formula?
AlO
Al₂O₃
Al₃O₂
AlO₂
After crisscrossing, if you get Pb₂S₄, what should you do?
Leave it as is
Simplify to PbS₂
Double it
Add more atoms
What is the formula for "calcium phosphate"?
CaPO₄
Ca₃(PO₄)₂
Ca(PO₄)₃
Ca₂PO₄
What is the formula for "magnesium perchlorate"?
What is the formula for "hypochlorous acid"?
HClO
HClO2
HClO3
HClO4
What is the formula for "nitrous acid"?
HNO
HNO2
HNO3
H2NO2
What is the formula for "diphosphorus pentoxide"?
PO5
P2O5
P5O2
P2O4
Which correctly describes why ionic compounds are called "salts"?
They all contain sodium
General shorthand term for ionic compounds
They're all soluble
They all taste salty
If an ionic compound has oxygen as the anion, it's called:
(a)
What is the difference between "electrolyte" and "nonelectrolyte"?
Electrolyte conducts, nonelectrolyte doesn't
Electrolyte has ions, nonelectrolyte doesn't
Electrolyte is ionic, nonelectrolyte is covalent
All of the above
In the crisscross method, what happens to the charges?
They become subscripts
They're dropped
They're written as + and -
They're ignored
Which correctly describes charge notation?
1+ and +1 are the same
1+ is preferred
+1 is preferred
Both A and B
What is the relationship between bond length and bond strength?
Shorter = stronger
Longer = stronger
No relationship
Depends on the atoms
Which correctly describes the process of ion formation?
Atom gets extra or less electrons during bonding
Goes to that charge number
Different from normal ion (process during bonding)
All of the above
Why can't electrons move through solid ionic compounds?
Compare BeCl₂ and H₂O. Both have 2 bonding domains, but BeCl₂ is linear while H₂O is bent. Why?
A) Be is smaller
B) H₂O has lone pairs that compress the angle
C) BeCl₂ has no lone pairs, H₂O has 2 lone pairs
D) Both B and C
Compare SO₂ and CO₂. Why is SO₂ polar but CO₂ is nonpolar?
SO₂ has more atoms
SO₂ has a lone pair (bent), CO₂ has no lone pairs (linear)
S is more electronegative
CO₂ has double bonds
Compare CH₃F and CH₄. Which has higher boiling point and why?
CH₄ (more atoms)
CH₃F (has dipole-dipole, CH₄ only has LDF)
They're equal
CH₄ (stronger bonds)
Compare the halogens F₂, Cl₂, Br₂, I₂. The trend from gas to solid is due to:
Increasing atomic number
Increasing electrons = stronger LDF
Increasing size
All of the above
Why does CH₃OH dissolve in water but CH₄ doesn't?
CH₃OH is polar (has H-bonds with water)
CH₄ is nonpolar (only weak LDF with water)
Like dissolves like
Compare molten NaCl and solid NaCl. Why does molten conduct but solid doesn't?
Molten has more ions
Solid: ions locked in lattice; Molten: lattice broken, ions free
Temperature affects conductivity
Both B and C
Which correctly explains the complete process of water dissolving NaCl?
Water breaks lattice → ions separate → ions surrounded by water
Water's polarity attracts ions → breaks lattice → ions free to move
Hydration occurs → dissociation occurs → conductivity possible
All of the above describe parts of the process
Compare H₂O and H₂S boiling points. The difference is primarily due to:
Molecular size
H₂O has hydrogen bonds, H₂S has only dipole-dipole
H₂O is more polar
All contribute, but B is primary
