2.9: End of Chapter Problems

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Page ID: 435559

Deboleena Roy (American River College)
American River College

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Atoms

1. What are the charges and the relative masses of the three subatomic particles?

2. Describe the structure of an atom in terms of its protons, neutrons, and electrons.

Elements

1. What is an element? Why are chemical symbols so useful? What is the source of the letter(s) for a chemical symbol?

2. Write the chemical symbol for the following elements.

bromine

carbon

calcium

gold

manganese

magnesium

neon

nitrogen

silver

3. What element is represented by each chemical symbol?

Atomic Number, Mass Number, Atomic Symbol, and Isotopes

1. What is the number of protons in the nucleus of each element?

aluminum

iron

carbon

sodium

oxygen

chlorine

2. How many electrons are present in the atoms of each element?

sulfur

iron

argon

magnesium

potassium

iodine

3. How many protons, electrons, and neutrons are in each atom?

Atomic Symbol.png

4. Why is the atomic number so important to the identity of an atom?

5. What is the relationship between the number of protons and the number of electrons in an atom?

6. How do isotopes of an element differ from each other?

7. What is the mass number of an element?

8. Which are isotopes? Explain.

9. Complete the following table.

Number of Protons	Number of Neutrons	Element Name

95	153
	21	potassium

Atomic Weight

1. In nature the element oxygen exists as three different isotopes, O-16, O-17, and O-18. Which isotope predominates? Explain.

2. Copper exists as a mixture of 2 isotopes.⁶³Cu and ⁶⁵Cu. Which isotope predominates?

3. Define atomic mass. Why is it considered a weighted average?

4. a. What is an atomic mass unit?

b. What is the atomic weight of zinc in atomic mass units?

c. What is the atomic weight of barium in atomic mass units?

Periodic Table

5. How are the elements organized into the periodic table?

6. Looking at the periodic table, where do the following elements appear?

the metals

the nonmetals

the halogens

the transition metals

the noble gases

7. Describe the trends in atomic radii as related to an element’s position on the periodic table.

8. Using the periodic table, which atom is larger? Explain.

N or Bi

Mg or Cl

Li or F

Na or K

9. a. A potassium atom has ____ core electrons and ____ valence electrons.

b. A silicon atom has ____ core electrons and ____ valence electrons.

c. How many total and valence electrons are in a neutral phosphorus atom?

d. How many total, valence, and core electrons are there in a neutral xenon atom?

Mole-Mass Conversions

1. How many moles are present in 100.0 g of Al?

2. How many moles are present in 25.5 g Na?

3. What is the mass of 8.603 mol of Fe metal?

4. What is the mass of 0.552 mol of Ag metal?

Physical & Chemical Properties

1. Which of the following is a chemical property of iron?

Iron corrodes in moist air

Density = 7.874 g/cm³

Iron is soft

pure iron melts at 1808 K

2. Which of the following is a physical property of matter?

corrosiveness

pH (acidity)

density

flammability

3. Which of the following is a chemical property?

flammability

melting point

boiling point

density

4. Label each of the following changes as a physical or chemical change.

a. Boiling water

b. A nail rusting

c. A green solution and colorless solution are mixed. The resulting mixture is a solution with a pale green color.

d. Two colorless solutions are mixed. The resulting mixture has a yellow precipitate.

e. A mirror is broken.

f. An iron nail corroded in moist air

g. Copper metal is melted.

h. A catalytic converter changes nitrogen dioxide to nitrogen gas and oxygen gas.

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