1. Specific Question Types
In terms of
State the relationship
Compare

2. In Terms Of
When answering these questions, your answer must be in terms related to what they ask, not always those exact terms

3. 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

4. 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

5. 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.

6. 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.

7. 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.

8. 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.

9. 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.

10. 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

11. 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

12. Example #10
Explain, in terms of subatomic particles, why the radius of a chloride ion is larger than the radius of a chlorine atom.
It has more electrons
The ion has more electrons
Which one?

13. 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

15. In terms of … Particle Arrangement Subatomic Particles
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

16. In terms of … Electrons Electronegativity Collision Theory
Electrons are shared/transferred/lost/gained
Electronegativity
which is higher/lower?
Use electronegativity difference (Bonds)
Collision Theory
Use the word “collisions” in your answer

17. In terms of … LeChatelier’s Principle Energy flow
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

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19. 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)

20. 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

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22. Compare… When comparing two things
State which one is larger/smaller… than the other
Mention both properties being compared

23. 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

24. 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.

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