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Periodic Table Review Flashcards | StudBud
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Periodic Table Review
Periodic Table Review
30 terms
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A review on the periodic table, focused on trends, element families, and periods/groups.
Flashcards
30 cards
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Practice quiz
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Questions
30
Answers
1
Rank these elements by ATOMIC RADIUS (small to big): carbon, aluminum, oxygen, potassium
O, C, Al, K
C, Al, O, K
Al, K, C, O
O, Al, K, C
2
How many valence electrons are in boron (B)?
3
1
4
2
3
What is the correct period, group, and block for silver (Ag)?
Period 6, group 10, d block
Period 7, group 11, p block
Period 5, group 11, d block
Period 1, group 5, s block
4
A valence electron is:
An electron in the nucleus
An electron in the outermost shell
An electron that will not bond
An electron in the innermost shell
5
Atomic radius is:
The width of the nucleus
1/2 the distance b/w the nuclei of 2 atoms of the same type
The distance from one side to the other of an atom
The size of an electron
6
Which sequence correctly places the elements in order of increasing ionization energy?
H, Be, Al, Ga
I, Br, Cl, F
H, Li, Na, K
O, S, Se, Te
7
Which block contains the transition metals?
s
f
d
p
8
Which element in Group 16 has the greatest tendency to gain electrons?
Se
O
S
Te
9
How many valence electrons are in fluorine (F)?
5
7
4
6
10
Ionization energy is
The amount of energy needed to remove an e- from an atom
The tendency of an atom to attract electrons
The ability to bond
The size of an atom
11
Group ____ contains the alkaline earth metals.
17
18
2
1
12
As atomic radius increases, ionization energy generally
Explodes
Stays the same
Increases
Decreases
13
Which properties are most common in nonmetals?
High ionization energy, high electronegativity
Low ionization energy, high electronegativity
Low ionization energy, low electronegativity
High ionization energy, low electronegativity
14
Electronegativity is:
The tendency of an atom to attract electrons
The energy it takes to remove an electron from an atom
The size of an atom
The tendency of an atom to repel electrons
15
Which has the greater ionization energy?
Ar
P
K
Na
16
The ability of carbon to attract electrons is:
Greater than that of nitrogen and oxygen
Less than that of oxygen and nitrogen
Less than that of nitrogen, but greater than that of oxygen
Greater than that of nitrogen, but less than that of oxygen
17
This element family is extremely reactive.
Halogens
Alkaline Earth metals
Alkali metals
Noble gases
18
Which of the following is not a TYPE of element?
Metalloid
Metal
Nonmetal
Alkali Metal
19
The less an element attracts electrons, the lower its:
Electronegativity
Atomic radius
Valence electrons
Ionization energy
20
Which is a property of metalloids?
Poor conductor of electricity
Mostly gases
Good conductor of heat
Characteristics depend on conditions
21
Which of the following is a characteristic of halogens?
All liquids
All toxic
All solids
Unreactive
22
Xenon belongs to which family?
Alkali Earth metals
Halogens
Metalloids
Noble gases
23
Which sequence of elements is arranged in order of decreasing atomic radii?
Al, Si, P
Li, Na, K
Cl, Br, I
N, C, B
24
Which electron configuration represents a transition metal?
1s22s22p5
[Ar]3d104s24p6
[Ar]3d5
[Ne]3s2
25
Rank the following elements by increasing ELECTRONEGATIVITY: sulfur, oxygen, neon, aluminum.
Al, S, O, Ne
Al, Ne, O, S
S, O, Ne, Al
O, S, Ne, Al
26
The elements Ca & Sr have similar chemical properties because they both have the same
Atomic number
Number of valence electrons
Number of completely filled sublevels
Mass number
27
The Group 17 element with the highest electronegativity is
Bromine
Iodine
Chlorine
Fluorine
28
As each successive element in Group 15 increases in atomic number, the atomic radius:
Decreases
Stays the same
Explodes
Increases
29
Ionization energy increases
From right to left across the periodic table
Diagonally to the lower left
Diagonally to the lower right
From left to right across the periodic table
30
Oxygen belongs to which family?
Metalloids
Metals
Nonmetals
Halogens
