AnswersTX-Integrated Physics and Chemistry A-CRUnit Test

Metals Answers

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1
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This is how fluorine appears in the periodic table.

Question illustration
A
the atomic number
B
the atomic mass
C
the mass of neutrons
D
the number of neutrons
2
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The element phosphorus is located to the right of the element magnesium along the same period in the periodic table.Which best describes the relationship of the elements?

A
Magnesium has a larger atomic number.
B
Phosphorus has a larger atomic mass.
C
Magnesium is in the same category as phosphorus.
D
Phosphorus has similar chemical properties as magnesium.
3

While looking at calcium (Ca) on the periodic table, a student needs to find an element with a greater atomic mass in the same period. Where should the student look?

A
directly up
B
directly down
C
directly to the left
D
directly to the right
4

Based on the information in the table, which elements are most likely in the same periods of the periodic table?

Question illustration
A
Boron and carbon are likely together in one period because they have very close atomic masses, while gallium and germanium are likely together in another period because they have very close atomic masses.
B
Aluminum, boron, and carbon are likely together in one period because they were first isolated in the first half of the 1800s, while gallium and germanium are likely together in another period because they were first isolated in the second half.
C
Boron and carbon are likely together in one period because they each end in “-on,” while aluminum, gallium, and germanium are likely together in another period because they each end in “-ium.”
D
Aluminum, boron, and gallium are likely together in one group because they have the same number of valence electrons, and carbon and germanium are likely together in another group because they have the same number of valence electrons.
5

This is how zirconium appears in the periodic table.

Question illustration
A
40
B
51
C
91
D
131
6

Part of one row of the periodic table is shown.

Question illustration
A
tin (Sn)
B
antimony (Sb)
C
tellurium (Te)
D
iodine (I)
7

While developing his periodic table, Dmitri Mendeleev broke his own rule and placed the element tellurium before iodine in the group. He did this even though tellurium's atomic mass was known to be greater than iodine's. In his notes, Mendeleev stated that he expected tellurium to have a lower atomic mass than iodine. However, all measurements continue to show that tellurium has a greater atomic mass than iodine even though tellurium acts like it has a lower atomic mass.

A
Mendeleev observed that tellurium has chemical properties like other elements in its group, and he did not know that neutrons cause the greater atomic mass.
B
Iodine isotopes usually have more neutrons than tellurium isotopes, but only the protons affect the properties that Mendeleev could have observed.
C
Mendeleev observed that tellurium and iodine both had very similar chemical properties, but he did not know that iodine atoms have more electrons.
D
Iodine atoms always have more protons than tellurium atoms, but Mendeleev only weighed elements without observing any other properties.
8

Elements in group 2 are all called alkaline earth metals. What is most similar about the alkaline earth metals?

A
how many protons and neutrons they have
B
which chemical properties they have
C
how many total electrons they have
D
which period they are most often found in
9

This is how osmium appears in the periodic table.

Question illustration
A
76
B
114
C
190
D
266
10

Which two chemists organized elements based on properties such as how the elements react or whether they are solid or liquid?

A
Lavoisier and Mendeleev
B
Döbereiner and Newlands
C
Newlands and Mendeleev
D
Lavoisier and Döbereiner

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