First Unit Review
Go to the Answer Key
- What is an element?
- What is a compound?
- State the difference between a physical change and a
- Review your sig figs and how to use them in calculations.
- a) A substance was found to have a mass of 35.94 g and a
volume of 3.18 mL. What is its density?
b) A sample of aluminum (density = 2.78 g/mL) was found
to have a mass of 72.98 grams. What is its volume?
- Make the following conversions: a) 380 seconds to hours
b) 2500 mL/min to L/second
- State the four principles of Dalton's atomic theory.
- List the three main subatomic particles. Give their
symbol, charge, approximate relative mass, and location
in the atom.
- Describe Rutherford's experiment, his results, and
conclusions he drew from them.
- What is an isotope?
- Describe J.J. Thomson's experiment and his results.
- Fill in the following table. (It includes ions, which are
in a later chapter, but might as well cover it now.)
or Ion Name
||Element or Ion
||# of p+
||# of e-
||# of no
- The four isotopes of lead are 122Pb with an
abundance of 1.37%, 124Pb with an abundance of
26.26%, 125Pb in 20.82% abundance, and 126Pb
in 51.55% abundance. What is the atomic mass of lead?
- What was the difference between the atom as described by
Thomson, Rutherford, Bohr, and the quantum mechanical
- List the four types of sublevels that an electron can
occupy. State how many orbitals are in each sublevel and
how many electrons can occupy that sublevel.
- State the Aufbau principle, the Pauli exclusion
principle, and Hund's rule.
- Write electron configurations for the following elements:
a) Na b) Kr c) Ta
- List the colors of the spectrum in order of increasing
- What is the wavelength, in nm, and the energy of light
whose frequency is 4.14 x 1014 Hz?
- Explain why we see lines in an atomic spectrum. A diagram
may be useful.
- Identify each of the following as metals, nonmetals, or
a) sodium b) carbon c) radium d)
silicon e) xenon
- Explain how calcium forms a +2 cation. Name the ion.
- Explain how phosphorus forms a -3 anion. Name the ion.
- What is the difference between a molecular compound and
an ionic compound?
- KNOW YOUR POLYATOMIC IONS!
- Write formulas for the following compounds. State whether
they are molecular or ionic.
a) calcium iodide b) phosphorus pentachloride
c) ammonium sulfide
d) copper (I) hydrogen phosphite e) dinitrogen
pentoxide f) tin (IV) oxalate
- Name the following compounds:
a) KMnO4 b) SnCr2O7
c) S2O3 d) NaNO3
- How many molecules in 42.99 grams of carbon dioxide?
- How many grams are in one mole of calcium hydrogen
- How many grams in 4.39 moles of magnesium nitrate?
- How many liters are in 2.3 grams of sulfur dioxide gas at
- Determine the number of moles in 182.49 L of hydrogen gas
- What is the molar mass of a gas which has a density of
2.86 g/L at STP?
- How many atoms of O are in 2.33 grams of nitrogen
- What is the percent carbon by mass in sucrose (C12H22O11)?
- A compound is composed of 58.8% C, 9.8% H, and 31.4% O.
a) Find its empirical formula.
b) What is its molecular formula if its molar mass is 204
- List the five types of reactions and briefly describe
- Why must an equation be balanced?
- Write and balance the following equations (finish if
needed). Identify each type.
a) carbon and oxygen react to form carbon monoxide
b) potassium chlorate decomposes to form potassium
chloride and oxygen
c) iron (III) chloride reacts with calcium hydroxide
d) magnesium reacts with silver nitrate
e) butane (C4H10) burns in air
f) potassium reacts with oxygen
- Write a balanced net ionic equation for each reaction.
a) lead (II) nitrate reacts with sodium chloride (lead
(II) chloride is a precipitate)
b) zinc is placed in hydrochloric acid solution
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