Week 7 Review AP Chemistry K-CHEMISTRY

Multiple Choice

This is an example of a __________ bond.

• non-polar covalent
• polar covalent
• ionic
• metallic

Reorder

Reorder the following steps for drawing lewis structures

• The Valence electrons

  charge - add/subtract if there is a charge

• Place the lower Electronegative atom in the centre and draw in bonds

• Add remaining electrons as Lone pairs (terminal atoms first).

• If any atoms dont have an Octet, use electrons to create double bonds.

• Check each atom has the same number of electrons as it started with (formal charge)

1

2

3

4

5

• 1
• 2
• 3
• 4
• 5

Multiple Choice

What is the molecular geometry of the compound described in the image?

• Tetrahedral

• Trigonal planar

• Linear

• Bent

Fill in the Blanks

Multiple Choice

Choose the correct shape for this molecule:

• Trigonal planar
• Trigonal pyramidal
• Tetrahedral
• Linear

a) Sulfur is bonded to one oxygen with a double bond, and the other three oxygens with single bonds.

b) All four S–O bonds are equivalent due to resonance.

c) The shape of the ion is tetrahedral.

d) Both b and c.

✅ Answer:

d) Both b and c.

​b) All four S–O bonds are equivalent due to resonance. c) The shape of the ion is tetrahedral.

Multiple Choice

Define the term resonance structure

• Delocalization of electrons in an atom
• Delocalization of π electrons within a molecule
• Spread of π electrons in an atom
• Spread of π electrons within a molecule

• Resonance means: when more than one valid Lewis structure can be drawn for a molecule/ion, the actual structureis a hybrid where electrons (usually π electrons or lone pairs) are delocalized across multiple bonds/atoms.

• • It is not confined to a single atom

Multiple Choice

What is the molecular geometry of the compound with 32 valence electrons and resonance that results in 4 equal S–O bonds?

• Linear

• Trigonal Planar

• Tetrahedral

• Octahedral

Multiple Choice

What shape would this have?

• Trigonal planar

• Pyramidal

• Tetrahedral

• Bent

Open Ended

Why is CO2 nonpolar?

Multiple Select

The shape of the carbon dioxide molecule allows it to be classified as

• polar.

• linear.

• nonpolar.

• charged.

Multiple Choice

A molecule of NH₃ has the shape pictured. What is true about the molecule?

• It has no lone pairs and is non polar

• It has one lone pair and is polar

• It has no lone pairs and is polar

• It has one lone pair and is non polar

Open Ended

Is CH₂Cl₂ polar or nonpolar?

Multiple Choice

Why is the molecule polar?

• There are nonbonding pairs on the central atom.

• There are different types of elements bonded to the central atom.

• There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

Multiple Choice

Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

Reorder

Reorder the following elements by increasing atomic radius.

• Hydrogen

• lithium

• sodium

• Potassium

• Rubidium

1

2

3

4

5

• 1
• 2
• 3
• 4
• 5

Multiple Choice

Which has a higher ionization energy.. N or As?

• N, because with more p+ in its nucleus it attracts e- more making them harder to remove.

• As, because with more p+ in its nucleus it attracts e- more making them harder to remove.

• As, because with less energy levels the ve- are closer to/ more attracted to the nucleus making them harder to remove.

• N, because with less energy levels the valence e- are closer to/ more attracted to the nucleus making them harder to remove.

Reorder

Put the following in order of increasing ionization energy: Strontium (Sr) , Aluminum (Al) , Indium (In)

• Strontium

• Indium

• Aluminum

1

2

3

• 1
• 2
• 3

Reorder

Reorder the following from lowest to highest electronegativity

• Cs

• Sr

• As

• P

• F

1

2

3

4

5

• 1
• 2
• 3
• 4
• 5

Reorder

Rank the following from lowest to highest electronegativity

• Mg

• Si

• P

• S

• Cl

1

2

3

4

5

• 1
• 2
• 3
• 4
• 5

Multiple Select

Which of these molecules exhibit London dispersion forces? (Select ALL that apply.)

• a

• b

• c

• d

Multiple Select

What kind of intermolecular force would you find between water (polar that has O and H hbond) and acetone (polarthat has O for hbond)?

(Check all that apply)

• ion-dipole

• H-bonds

• dipole-dipole

• london dispersion

• none

Multiple Choice

What type of intermolecular forces are present in a polar bond that does not have a hydrogen bond donor?

• Dipole-dipole

• London dispersion

• Hydrogen bonding

• Ionic bonding

Multiple Choice

What are the intermolecular forces (IMF) present in CH3OH?

• Hydrogen bonding

• Dipole-dipole interactions

• London dispersion forces

• All of the above

Poll

How confident do you feel about these topics now?

• Very confident
• Somewhat confident
• Not confident

Skills tested week 7 AP Chemistry Revision

unit 1

Periodic Trends – Atomic Radius

Periodic Trends – Ionization Energy

Periodic Trends – Electronegativity

unit 2

Lewis Diagrams

Resonance & Formal Charge

VSEPR & Bond Hybridization

Polarity of Bonds & Molecules

unit 3

• Identify types of IMF

• Rank IMF strength qualitatively.

• Relate IMF strength to boiling point / melting point / vapor pressure.

• Explain volatility and evaporation rate trends.

Skills tested week 7 AP Chemistry Revision