Chemistry Copper Lab

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Chemistry 11
Final Examination Review - Answers
Part A - True or False.
Indicate whether each of the following statements is true or false. Correct the false statements.

F

1. The mass of an electron is equal to the mass of a proton.

The mass of an electron is less than the mass of a proton.
T

2. The mass of a proton is approximately equal to the mass of a neutron.

T

3. The atomic number represents the number of protons in a nucleus.

T

4. The proton has a mass of approximately 1 u.

F

5. The difference in mass of isotopes of the same element is due to the different number of protons in the nucleus.

The difference in mass of isotopes of the same element is due to the different number of neutrons in the nucleus.

T

6. The isotope carbon-12 is used as the relative mass standard for the atomic mass scale.

F

7. The mass of the most common isotope of each element is listed on the periodic table.

The average mass of the naturally occurring isotopes of each element is listed on the periodic table.

Part B - Multiple Choice
D
A

1. A(n) __ is used to represent a compound.
a) symbol
b) equation

c) subscript

d) formula

2. ___ atoms or groups of atoms are called ions.
a) charged
b) diatomic

c) neutral

d) monatomic

A

3. For the formula of a compound to be correct, the algebraic addition of the charges on the atoms or ions in the compound must add up to __.
a) zero
b) one
c) two
d) four

D

4. Potassium bromide is an example of a(n) __ compound.
a) molecular
b) organic
c) polyatomic

B

d) ionic

5. The only common polyatomic ion that has a positive charge is the __ ion. a) phosphate
b) ammonium
c) sulfate
d) nitrate

Chemistry 11 Exam Review – Answers - Page 1

A
B
D

6. In the formula H2SO4, the number 4 would be called a(n) __. a) subscript
b) oxidation number
c) coefficient

d) charge

7. Which subatomic particle contributes the least to the mass of an atom? a) nucleon
b) electron
c) proton
d) neutron
8. In the free, or uncombined, state the number of protons in the nucleus of an element must equal the __.
a) mass number
c) mass number - atomic number
b) number of neutrons in the nucleus
d) number of electrons present

C

9. Which of the following ideas of the Bohr model is not retained in the modern theory of atomic structure?
a) Electrons can absorb or emit energy only in whole numbers of photons. b) Atoms have a central positively charged nucleus.
c) Electrons move around the nucleus as planets orbit the sun. d) Most of the volume of an atom is empty space.

B

10. Which of the following orbitals is spherical in shape?
a) 3p
b) 2s
c) 4d

d) 5f

11. The third energy level of an atom may have __ electro ns. a) 2
b) 18
c) 8

d) 32

B
C

12. How many sublevels are possible at the fourth energy level? a) 2
b) 3
c) 4

d) 18

A

13. Lustrous, malleable, ductile elements that are good conductors of electricity and heat are classified as __.
a) metals
b) nonmetals
c) metalloids
d) noble gases

C

14. The electron configuration of a certain element ends with 3p5. Which of the following describes its position in the periodic table?
a) period 5, group 13 b) period 3, group 15
c) period 3, group 17 d) period 5, group 15

B

15. Which of the following is an example of a metalloid?
a) iodine
b) boron
c) bromine

d) indium

16. The periodicity of the elements is basically a function of their __. a) nuclear stability
b) atomic numbers
c) mass numbers

d) none of these

17. An element with seven electrons in the outer level would be a __. a) metal
b) metalloid
c) noble gas

d) nonmetal

B
D
A

18. As the atomic number in a period increases, the degree of nonmetallic character __. a) increases
c) increases then decreases
b) decreases
d) remains the same
Chemistry 11 Exam Review – Answers - Page 2

B

19. Elements in a group have similar chemical...
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