General Chemistry 1 (and a little 2) Final Review 2

Definitions & Concepts

100

What is a physical change?

No new substance formed

200

Are fireworks a chemical or physical change?

Chemical

300

Define precision vs accuracy. 

Precision = consistency; accuracy = closeness to true value

400

What is atomic number?

Number of protons that defines the element

500

Which trend increases across a period: atomic radius or ionization energy? (Bonus 100 points: give the definitions of atomic radius and ionization energy)

Ionization energy

Bonus:

Atomic Radius - size of an atom, from center of nucleus to outer electron shell

Ionization Energy - energy required to remove an electron

Periodic Table Trends

100

Does atomic radius decrease or increase across a period?

Decrease

200

Is hydrogen a metal, metalloid, or nonmetal?

Nonmetal

300

Which is more electronegative: Cl or Br?

Cl

400

Which is bigger: Cl^- or Cl?

Cl^-

500

Write the electron configuration of Fe³⁺.

[Ar]3d⁵

Chemical Bonding

100

What type of bond shares electrons?

Covalent

200

What is the arrhenius acid definition?

Produces H⁺ in water

300

What is the Brønsted-Lowry base definition?

Proton acceptor

400

Does a precipitate form? BaCl₂ + Na₂SO₄

Yes, BaSO₄

500

Is this reaction redox, acid-base, or precipitation? 

HCl + NaOH → NaCl + H₂O

Acid-base

Math

100

What is the molarity of 2 moles in 1 L?

2M

200

(12.11+0.3) × (3.42/1.005) 

*pay attention to sig fig calculation rules

42.2

300

Empirical formula of 40% C, 6.7% H, 53.3% O

CH₂O

400

Calculate the bond order of the carbonate ion (CO₃^2-)

1.33

500

Chlorine has two naturally occurring isotopes:

• ³⁵Cl with a mass of 34.97 amu
• ³⁷Cl with a mass of 36.97 amu

The average atomic mass of chlorine is 35.45 amu.

What is the percent abundance of each isotope?

76% ³⁵Cl and 24% ³⁷Cl

General Chemistry 2 Topics

100

What is pH + pOH?

14

200

A gas occupies 2.50 L at 1.20 atm and 300 K.
How many moles of gas are present?

0.122 mol

300

For the reaction: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) ΔH<0

What happens to equilibrium if temperature is increased? What if pressure is increased?

Increase temperature = shifts left (endothermic direction favored). Increase pressure = shifts right (fewer moles of gas: 3 → 2)

400

For a reaction with K=10 and Q=0.1 what happens?

Shifts right

500

A reaction has the rate law: rate=k[A]²[B]. What happens to the rate if [A] is doubled and [B] is tripled? 

Rate increases by factor of 12