Name:___________________________________________
Block:______ Date:_______________
Electrons and Atomic Properties Practice Test
1. The electron configuration for an atom is 1s22s22p63s23p64s23d104p6. How many valence electrons does
this atom have?
(A) 18
(B) 8
(C) 6
(D) 36
2. The electron configuration for helium is 1s2. The “1” stands for….
(A) the orbital
(B) how many electrons helium has
(C) the energy level the electrons are in
(D) the shape of the area that the electron’s in 90% of the time
3. Whenever an electron in hydrogen electron promoted from a low energy level to a high energy level, it:
(A) Absorbs energy
(B) Jumps back to its excited state
(C) Gives off energy
(D) Collapses into the nucleus.
4. An atom composed of 8 protons, 10 electrons, and 8 neutrons is
a. 16O2+
b. 16O2c. 18O
d. 18O25. What does a group refer to on the periodic table?
a. a column
b. a row
c. a period
d. one element individually
6. Among the groups of elements listed below, which have the same number of energy levels?
a. Li, Na, K, Rb
b. Na, Mg, B, C
c. K, Ca, Rb, Sr
d. N, P, As, Sb
7. How many valence electrons does strontium (Sr) have?
a. 1
b. 2
c. 88
d. 38
8. Which of the following has the greatest electronegativity?
e. Calcium
f. Gallium
g. Barium
h. Thallium
9. Which of the following elements has the largest atomic radius?
a. Potassium
b. Sodium
c. Gallium
d. Krypton
10. Which of the following elements has an electron configuration that ends with p3?
a. Boron
b. Tin
c. Antimony
d. Neon
11. Which has the longest wavelength of the options below?
a. Infrared
b. Red
c. Green
d. Ultraviolet
12. Which of the following statements are true?
I. The longer the wavelength, the more energy
II. The longer the wavelength, the higher the frequency
III. The higher the frequency, the higher the energy
a) I only
b) I + II
c) III only
d) I + III
e) None of the above
For these 3 questions, match each element with the correct electron configuration. Some answers will not be
used.
A = 1s1
B = [Ar]4s23d6
C = [Kr]5s24d105p3
D = [Kr]5s2
E = [He]2s22p1
AB = [Ne]3s23p2
13. Sr _____
14. H _____
15. Si _____
16. Which of the following best explains why fluorine is more electronegative than boron?
A) Electronegativity is the measure of how negative an atom is.
B) Fluorine has more electrons than boron
C) Fluorine has a higher effective nuclear charge
D) Fluorine is smaller than boron.
17. Which of the following best explains why sodium is smaller than potassium?
A) Sodium has a higher nuclear charge
B) Sodium has fewer valence electrons
C) Sodium has a higher electronegativity
D) Sodium has fewer energy levels
18) Which of the following is NOT a difference between the Bohr model and quantum mechanical model.
a. Electrons are in orbits for the Bohr model and orbitals for the quantum mechanical model.
b. Electrons are in energy levels for the Bohr models and the quantum model doesn’t address energy.
c. The Bohr model and quantum models are the same
19) Which of the following groups will have similar properties?
a. Li, B, C, F
b. Na, Mg, Al, S
c. K, Ca, Rb, Sr
d. N, P, As, Sb
20) What is the valence energy level for S?
a. 3
b. 6
c. 16
d.4
Open Response:
1) Compare and contrast the Bohr and quantum mechanical atomic models.
2) Fill in the chart below
Element
Electron Config.
Valence level
Valence electrons
Be
Co
Pd
Sr
1s22s22p5
[Ar]4s23d5
3
3
4
7
6
8
3) Draw the Bohr model and box and arrow diagram for Calcium
Bohr Model
Box and Arrow Diagram
4) On the periodic table below draw arrows that describe the trends in electronegativity and atomic size
across a period and down a group. Below explain those trends in terms of effective nuclear charge and
electron shielding.