Measurements
Atoms n Moles
Light n Colors
Electrons/Periodic Trends
Ionic Compounds n Bonding
100

How many significant figures are in 0.00450?  

3 

100

How many neutrons are in ²³₁₁Na?

12 neutrons

100

Which type of electromagnetic radiation has the longest wavelength?

A. Ultraviolet
B. Microwaves
C. Gamma rays
D. X-rays

B. Microwaves

100

Which atom has the smallest atomic radius?

A. Sodium
B. Magnesium
C. Aluminum
D. Potassium

C. Aluminum

100

What is the correct formula for magnesium chloride?

MgCl₂

200

Calculate and report with the correct number of significant figures:
12.5 g + 3.24 g

15.7 g

200

An isotope undergoes alpha decay:

92238U→?+24He

What is the resulting Isotope?

 90234Th


200

A green light has a wavelength of 525 nm.

What is the frequency of this photon?

5.71×10^14 hz

200

Rank the following elements from greatest to least electron affinity:

  • Chlorine (Cl)
  • Sulfur (S)
  • Phosphorus (P)
  • Sodium (Na)

A. Cl > S > P > Na
B. S > Cl > P > Na
C. Na > P > S > Cl
D. Cl > P > S > Na

Cl > S > P > Na

200

What is the charge of an oxide ion?

O²⁻

300

A cyclist is traveling at 18 miles per hour. How many feet will they travel in exactly 15 seconds?

1 mile = 5280 ft

1 hr = 3600 sec

396 ft

300

An element has two isotopes:

  • Isotope A: 10.0 amu, 20% abundance
  • Isotope B: 11.0 amu, 80% abundance

What is the average atomic mass of the element?

10.8 amu

300

A photon has a wavelength of 450 nm. What is its energy?

4.42×10^−19 J

300

An electron is located in the n=4 energy level. Which of the following could represent a possible set of quantum numbers for this electron?

A. n=4, ℓ=2, mℓ=−1, ms=+1/2
B. n=4, ℓ=4, mℓ=0, ms=−1/2
C. n=4, ℓ=3, mℓ=4, ms=+1/2
D. n=4, ℓ=1, mℓ=2, ms=−1/2

A. n=4, ℓ=2, mℓ=−1, ms=+1/2

300

What is the correct name for FeCl₃?

Iron(III) chloride

400

Calculate and report your answer using the correct number of significant figures:

(12.5+3.42)×2.0


32

400

What are the three laws that correlate to the atom?


Law of Constant Composition

Law of Multiple Proportions

Law of Conservation of Mass

400

Determine the wavelength of an electron traveling at a speed of:

3.00×10^6 m/s 

m = 9.109×10^−31 kg

2.42x10^-10 m or 0.242 nm

400

Write the electron configuration for sulfur (S) in both forms:

  1. Full electron configuration:

  2. Noble gas shorthand configuration:
  • Full: 1s^2 2s^2 2p^6 3s^2 3p^4
  • Shorthand: [Ne]3s^2 3p^4
400

Which compound would be expected to have the greatest magnitude of lattice energy?

A. NaCl
B. KCl
C. MgO
D. MgCl₂

C. MgO

500

A camping stove uses a fuel that releases 42 kJ of energy per gram. A fuel canister holds 2.50 gallons of fuel with a density of 0.75 g/mL. How much energy, in joules, can the canister provide?

1g = 3785.41 mL

2.98×10^8 J

500

Caffeine has the formula C₈H₁₀N₄O₂. A cup of coffee contains 0.0150 moles of caffeine. How many moles of nitrogen atoms are present in 3 cups of coffee?

0.180 mol

500

Calculate the wavelength of light emitted when a hydrogen electron transitions from n = 5 to n = 2.

434 nm

500

Write the electron configuration for copper (Cu)

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^10

500

Consider the following steps in the formation of NaCl(s):

  • Na(s) → Na(g) = +108 kJ/mol
  • Na(g) → Na⁺(g) + e⁻ = +496 kJ/mol
  • ½Cl₂(g) → Cl(g) = +122 kJ/mol
  • Cl(g) + e⁻ → Cl⁻(g) = −349 kJ/mol
  • Na⁺(g) + Cl⁻(g) → NaCl(s) = ?

The overall enthalpy of formation of NaCl(s) is −411 kJ/mol.

What is the lattice energy?

-788 kj/mol

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