Download Pre-AP Chemistry Exam 4 - Harding Charter Preparatory High School

Name_______________________________________Date__________________________Period__________
Pre-AP Chemistry Exam 4
Matching
Match each item with the correct statement below.
a. atomic orbital
d. ground state
b. aufbau principle
e. Pauli exclusion principle
c. electron configuration
f. Heisenberg uncertainty principle
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1.
2.
3.
4.
5.
6.
region of high probability of finding an electron
states the impossibility of knowing both velocity and position of a moving particle at the same time
lowest energy level
tendency of electrons to enter orbitals of lowest energy first
arrangement of electrons around atomic nucleus
each orbital has at most two electrons
Match each item with the correct statement below.
a. atomic emission spectrum
d. photon
b. frequency
e. quantum
c. wavelength
f. spectrum
____ 7. discrete bundle of electromagnetic energy
____ 8. energy needed to move an electron from one energy level to another
____ 9. number of wave cycles passing a point per unit of time
____ 10. distance between wave crests
____ 11. separation of light into different wavelengths
____ 12. frequencies of light emitted by an element
Match each item with the correct statement below.
a. electronegativity
f.
b. ionization energy
g.
c. atomic radius
h.
d. metal
i.
e. transition metal
j.
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13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
periodic law
cation
period
group
electrons
horizontal row in the periodic table
vertical column in the periodic table
A repetition of properties occurs when elements are arranged in order of increasing atomic number.
type of element that is a good conductor of heat and electric current
type of element characterized by the presence of electrons in the d orbital
one-half the distance between the nuclei of two atoms when the atoms are joined
type of ion formed by Group 2A elements
subatomic particles that are transferred to form positive and negative ions
ability of an atom to attract electrons when the atom is in a compound
energy required to remove an electron from an atom
Multiple Choice
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Name_______________________________________Date__________________________Period__________
Identify the letter of the choice that best completes the statement or answers the question.
____ 23. What is the name given to the electrons in the highest occupied energy level of an atom?
a. orbital electrons
c. anions
b. valence electrons
d. cations
____ 24. The octet rule states that, in chemical compounds, atoms tend to have ____.
a. the electron configuration of a noble gas
b. more protons than electrons
c. eight electrons in their principal energy level
d. more electrons than protons
____ 25. What is the electron configuration of the oxide ion (O )?
a. 1s 2s 2p
c. 1s 2s
b. 1s 2s 2p
d. 1s 2s 2p
____ 26. Under what conditions can potassium bromide conduct electricity?
a. only when melted
b. only when dissolved
c. only when it is in crystal form
d. only when melted or dissolved in water
____ 27. Which of the following is NOT a characteristic of most ionic compounds?
a. They are solids.
b. They have low melting points.
c. When melted, they conduct an electric current.
d. They are composed of metallic and nonmetallic elements.
____ 28. An ionic bond is a bond between ____.
a. a cation and an anion
c. the ions of two different metals
b. valence electrons and cations
d. the ions of two different nonmetals
____ 29. Why do atoms share electrons in covalent bonds?
a. to become ions and attract each other
b. to attain a noble-gas electron configuration
c. to become more polar
d. to increase their atomic numbers
____ 30. Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in
diatomic oxygen molecules?
a. unvalenced pair
c. inner pair
b. outer pair
d. unshared pair
____ 31. Each period in the periodic table corresponds to ____.
a. a principal energy level
c. an orbital
b. an energy sublevel
d. a suborbital
____ 32. To what category of elements does an element belong if it is a poor conductor of electricity?
a. transition elements
c. nonmetals
b. metalloids
d. metals
____ 33. Atomic size generally ____.
a. increases as you move from left to right across a period
b. decreases as you move from top to bottom within a group
c. remains constant within a period
d. decreases as you move from left to right across a period
____ 34. Which of the following elements has the smallest first ionization energy?
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Name_______________________________________Date__________________________Period__________
a. sodium
c. potassium
b. calcium
d. magnesium
____ 35. Which of the following elements has the lowest electronegativity?
a. lithium
c. bromine
b. carbon
d. fluorine
____ 36. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
Short Answer
37. Give the electron configuration for a neutral atom of selenium, (34Se).
38. Draw an orbital diagram showing all the electrons as arrows in a neutral atom of phosphorous. Don’t forget to
label your boxes with the appropiate sublevels.
39. Draw a Lewis structure (electron dot structure) for the oxygen atom.
40. Draw a Lewis structure for methane (CH4).
41. Which group in the periodic table is known as the noble gases?
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Name_______________________________________Date__________________________Period__________
42. Is nitrogen a metal or nonmetal? What group is it in? What charge will nitrogen have when it becomes an
ion?
Numeric Response
43. How many electrons are in the highest occupied energy level of a neutral chlorine atom?
44. How many unpaired electrons are in there in a neutral nitrogen atom?
45. What is the charge of a particle having 9 protons and 10 electrons?
46. How many electrons are shared in a single covalent bond?
47. How many unshared pairs of electrons does the oxygen atom in water (H2O) possess?
48. How many electrons are shared in a double covalent bond?
49. How many electrons are there in the highest occupied energy level of atoms in Group 5A elements?
Essay
50. Describe the trends in the atomic size of elements within groups and across periods in the periodic table.
Provide examples.
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Name_______________________________________Date__________________________Period__________
Pre-AP Chemistry Exam 4
Answer Section
MATCHING
1. ANS: A
2. ANS: F
3. ANS: D
4. ANS: B
5. ANS: C
6. ANS: E
7. ANS: D
8. ANS: E
9. ANS: B
10. ANS: C
11. ANS: F
12. ANS: A
13. ANS: H
14. ANS: I
15. ANS: F
16. ANS: D
17. ANS: E
18. ANS: C
19. ANS: G
20. ANS: J
21. ANS: A
22. ANS: B
MULTIPLE CHOICE
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
B
A
B
D
B
A
B
D
A
C
D
C
A
A
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Name_______________________________________Date__________________________Period__________
SHORT ANSWER
37. ANS:
1s 2s 2p 3s 3p 3d 4s 4p
38. ANS:
1s2
2s2
2p6
3s2
3p6
39. ANS:
The chemical symbol for oxygen with two single dots in two quadrants and two pairs of dots in two quadrants.
Six dots total.
40. ANS:
Carbon with one hydrogen in each of carbons quadrants. One line is used to connect each hydrogen to carbon.
41. ANS:
8A
42. ANS:
nonmetal, 5A, 3NUMERIC RESPONSE
43. ANS:
7
44. ANS:
3
45. ANS:
1
46. ANS:
2
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Name_______________________________________Date__________________________Period__________
47. ANS:
2
48. ANS:
4
49. ANS:
5
ESSAY
50. ANS:
Atomic size increases with increasing atomic number within a group. For example, sodium atoms are larger
than lithium atoms, and potassium atoms are larger than sodium atoms. Atomic size decreases with increasing
atomic number across a period. For example, lithium atoms are larger than beryllium atoms, and beryllium
atoms are larger than boron atoms.
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