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Unit 4 On Level Test

Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
Which of the following is a pure substance?
a.
all of the above
c.
Hydrogen Fluoride and Potassium Oxide (HF + K2O )
b.
Magnesium (Mg)
d.
Sodium Chloride and water (NaCl + H2O )
 

 2. 
Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a.
Pt
b.
V
c.
Kr
d.
Li
 

 3. 
Which of the following elements has the smallest atomic radius?
a.
S
b.
Li
c.
K
d.
O
 

 4. 
Which of the following changes to a metal is a chemical change?
a.
rusting
b.
polishing
c.
melting
d.
bending
 

 5. 
Which of the following is considered a physical property of a substance?
a.
products of decomposition
b.
reaction with an acid
c.
malleability
d.
ability to oxidize
 

 6. 
Sodium, mercury, argon and neon are used in the production of lamps. There are fewer safety guidelines regarding the handling of neon and argon than for mercury and sodium. Which of the following best describes the properties of elements in the same family as neon and argon?
a.
Solid at room temperature
c.
Mostly unreactive
b.
Solid at room temperature and mostly unreactive with strong acids
d.
Gaseous at room temperature and highly reactive
 

 7. 
Which of the following statements is an accurate description of the ionization energies of elements within the periodic table?
a.
The ionization energy of magnesium is greater than that of sulfur.
c.
The ionization energy of krypton is greater than that of neon.
b.
The ionization energy of iodine is greater than that of fluorine.
d.
The ionization energy of sulfur is greater than that of potassium.
 

 8. 
Chemist can identify the composition of some unknown salts by conducting a flame test. When potassium salts are heated in a flame, a purple color is observed. What is the electron configuration of a Potassium (K) atom?
a.
1s2 2s2 2p6 3s2 3p6 4s1 
c.
1s2 2s2 2d6 3s2 3p6 4s2
b.
1s2 2s2 2p6 3s2 3p6 4d1     
d.
1s2 2s2 2p6 3s2 3p6 3d1
 

 9. 
What element has the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d104p65s24d8 ?
a.
Platinum (Pt)     
c.
Nickel (Ni)     
b.
Tin (Sn)
d.
Palladium (Pd)
 

 10. 
Which of the following statements is true?
a.
Electrons are negatively charged and have a mass of 1 amu.
b.
The nucleus of an atom is positively charged and never has a mass of 1 amu.
c.
Neutrons are negatively charged and have a mass of 1 amu.
d.
Protons are positively charged and have a mass of 1 amu.
 

 11. 
One of the wavelengths emitted by hydrogen atoms is
6.56 x 10-7 m. Calculate the frequency if the speed of light is 3.00 x 108 m/s..
a.
4.57 x 1014 Hz
c.
1.97 x 1014 Hz
b.
4.57 x 10-7 Hz
d.
4.57 x 10-6 Hz
 

 12. 
Which of the following factors contributes to the increase in ionization energy from left to right across a period?
a.
an increase in the shielding effect
b.
fewer electrons in the highest occupied energy level
c.
an increase in the number of protons
d.
an increase in the size of the nucleus
 

 13. 
As the wavelength of a wave increases, which is also TRUE?
a.
the frequency increases
c.
the frequency decreases
b.
planks constant increases
d.
the energy increases
 

 14. 
A sample of Element X is found to contain 72.15% of isotope type 1 (84.9118 amu) and 27.85% of isotope type 2 (86.9092 amu). Calculate the average atomic mass.
a.
86.21 amu
c.
85.47 amu
b.
86.49 amu
d.
85.13 amu
 

 15. 
As wavelength increases, what happens to Frequency and Energy?
a.
Frequency decreases, Energy increases
c.
Both Decrease
b.
Both Increase
d.
Frequency increases, Energy decreases
 

 16. 

What does the 3 represent in the following electron configuration, 1s2 2s2 2p6 3s2 3p6?
a.
Energy level of electrons
c.
Electrons
b.
Orbitals
d.
Sublevel
 

 17. 
An example of an extensive property of matter is
a.
mass.
b.
hardness.
c.
temperature.
d.
pressure.
 

 18. 
Which of the following describes the ability of a metal to be drawn into wires or be bent?
a.
malleable
c.
ductility
b.
conductivity
d.
soluble
 

 19. 
What is the maximum number of orbitals in the p sublevel?
a.
5
b.
2
c.
3
d.
4
 

 20. 
How many electrons are required to fill the 3rd energy level with the maximum number of electrons?
a.
2
c.
8
b.
32
d.
18
 

 21. 
Where in an atom is MOST of its mass found?
a.
in electron clouds
c.
in the f orbital
b.
in the nucleus
d.
in the 1s and 2s orbitals
 

 22. 
mc022-1.jpg

Which of the waves above has the highest energy?
a.
Microwave
c.
Infrared
b.
Gamma
d.
Ultraviolet
 

 23. 
What is the Noble Gas electron configuration for an atom of Germanium (Ge)?
a.
[Kr] 4s2 3d10 4p2     
c.
[Ar] 4s2 4d10 4p2
b.
[Ar] 4s2 3d10 4p2
d.
[Kr] 4s2 4d10 4p2
 

 24. 
As the atomic number increases within a group of elements, the atomic radius usually --
a.
decreases
c.
increases
b.
remains the same as the one above it
d.
decreases, then increases
 

 25. 
In which of the following is the number of neutrons correctly represented?
a.
mc025-1.jpgAs has 108 neutrons.
b.
mc025-2.jpgU has 146 neutrons.
c.
mc025-3.jpgF has 0 neutrons.
d.
mc025-4.jpgMg has 24 neutrons.
 

 26. 
Brass is an alloy made of copper and zinc.  To make brass copper is mixed with zinc when both metals are at the liquid state.  During the mixing process no chemical reaction takes place. After mixing, brass appears to be uniform throughout.  Brass must be a(n):
a.
heterogenous mixture
c.
homogenous mixture
b.
pure substance
d.
an element
 

 27. 
What is the electron configuration for Manganese (Mn), atomic number 25?
a.
1s2 2s2 2p6 3s2 3p6 4s2 3d10
c.
1s2 2s2 2p6 3s2 3p6 4s2 3d5
b.
1s2 2s2 2p6 3s2 3p6
d.
1s2 2s2 2p6 3s2 3p6 4s2
 

 28. 
How many valence electrons are in a silicon atom?
a.
8
b.
6
c.
4
d.
2
 

 29. 
A red light is measured to have a wavelength of 6.71 x 10-7 m. Given the speed of light (3.00 x 108 m/s) and Planck’s constant (6.63 x 10-34 Js), calculate the energy of one photon of this light.
a.
1.48 x 10-18 J
c.
2.96 x 10-19 J
b.
4.42 x 10-3 J
d.
1.33 x 10-18 J
 

 30. 
How many valence electrons are surrounding an element with the following electron configuration: 
1s2 2s2 2p6 3s2 ?
a.
3
c.
12
b.
2
d.
6
 



 
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