Specific Question Types
In terms of
 State the relationship
 Compare

In Terms Of

When answering these questions, your
answer must be in terms related to what
they ask, not always those exact terms
Example #1
2Na(s) + Cl2(g) → 2NaCl(s)
 Explain, in terms of electrons, why the bonding
in NaCl is ionic.

Because Na is a metal and Cl is a nonmetal
 In terms of electrons, the bonding in NaCl is
ionic because electrons are transferred. Na is
giving an electron to Cl.
 Electrons are transferred

Example #2

State, in terms of the number of subatomic particles,
one similarity and one difference between the atoms of
these isotopes of neon.
They all end with .99, but have different percentages.
 In terms of the number of subatomic particles, they are
similar because they have the same number of protons
and they are different because they have a different
number of neutrons.
 Same number of protons, different number of neutrons

Example #3

Explain, in terms of molecular polarity, why hydrogen
chloride is more soluble than methane in water at
20.°C and standard pressure.

Hydrogen chloride is more polar than methane
In terms of molecular polarity, hydrogen chloride is
more soluble than methane in water because hydrogen
chloride is polar, like water, and methane is nonpolar.
Hydrogen chloride is polar, methane is nonpolar.


Example #4

Explain, in terms of intermolecular forces, why ammonia
has a higher boiling point than the other compounds in
the table.

Ammonia has a lower boiling point because it has
stronger intermolecular forces.

Ammonia has a higher boiling point because it has
stronger intermolecular forces.
Example #5

Explain, in terms of electronegativity, why the H–F bond is
expected to be more polar than the H–I bond.

H-F has a higher electronegativity than H-I.

H-F has a larger electronegativity difference than H-I.
Example #6
Given the equation for a reaction at equilibrium:
 2SO2(g) + O2(g) → 2SO3(g) + energy
 Explain, in terms of LeChatelier’s principle, why the
concentration of SO2(g) increases when the
temperature is increased.


Equilibrium shifts towards the reactant side.
Example #7
Given the equation for a reaction at equilibrium:
 2SO2(g) + O2(g) → 2SO3(g) + energy
 Explain, in terms of collisions between molecules, why
increasing the concentration of O2(g) produces a
decrease in the concentration of SO2(g).


There are less collisions

There are more particles to collide.
Example #8

Explain, in terms of atomic structure, why germanium is
chemically similar to silicon.

They’re in the same group on the Periodic Table
In terms of atomic structure, germanium is chemically
similar to silicon because it has the same number of
valence electrons
They have the same number of valence electrons


Example #9

Explain, in terms of collision theory, why the
concentration of H2(g) begins to decrease immediately
after more H2(g) is added to the system.

There are less collisions.
More H2 means more particles colliding, more reactants
are converted to products, so the H2 concentration
decreases

Example #10

Explain, in terms of subatomic particles, why the
radius of a chloride ion is larger than the radius
of a chlorine atom.
Which one?
It has more electrons
 The ion has more electrons

Example #11

Explain, in terms of chemical reactivity, why the
elements in Group 18 on the modern Periodic Table
were not identified by Mendeleev at that time.

Group 18 elements have a full valence shell, so they
don’t react
In terms of …

Particle Arrangement
◦ Particles are arranged in a pattern, close together, far apart…

Subatomic Particles
◦ Use protons, neutrons , and/or electrons

Atomic Structure
◦ Mention energy levels, valence electrons, protons or neutrons or
electrons
In terms of …

Electrons
◦ Electrons are shared/transferred/lost/gained

Electronegativity
◦ which is higher/lower?
◦ Use electronegativity difference (Bonds)

Collision Theory
◦ Use the word “collisions” in your answer
In terms of …

LeChatelier’s Principle
◦ Equilibrium shifted to the left/right, towards reactants/products

Energy flow
◦ From which object to which object (hot  cold)

Strength of intermolecular forces
◦ Which is stronger/weaker?

Saturation
◦ Use saturated/unsaturated/supersaturated

Back
State the relationship

From a graph
◦ As the (x-variable) increases, the (y-variable)
(increases/decreases)

From data table
◦ As (pick a variable) (increases/decreases) the
(other variable) (increases/decreases)
Example #12

Describe the relationship between the concentration of
solution A and the time for the reaction to go to
completion.

As the time increases, concentration decreases

As concentration increases, the time decreases

Back
Compare…

When comparing two things
◦ State which one is larger/smaller… than the
other
◦ Mention both properties being compared
Example #13

Compare the boiling point of the NaCl solution at
standard pressure to the boiling point of H2O at
standard pressure.

NaCl has a higher boiling point

The solution has a higher boiling point than water
Example #14


At STP, iodine, I2, is a crystal, and fluorine, F2, is a gas.
Iodine is soluble in ethanol, forming a tincture of iodine.
A typical tincture of iodine is 2% iodine by mass.
Compare the strength of the intermolecular forces in a
sample of I2 at STP to the strength of the
intermolecular forces in a sample of F2 at STP.
 I2
has stronger intermolecular forces than F2.

Back