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Periodic Table Review
Periodic Table Review
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A #periodictable review for #honors #chemistry of Chapter 6 in their #modernchemistry textbook
Flashcards
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Questions
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Answers
1
Which is the best reason that the atomic radius generally increases with atomic # down a group?
the number of neutrons increases
the nuclear charge increases
the number of occupied energy levels increases
a new octet forms
2
When an electron is added to a neutral atom, a certain amount of energy is
always absorbed
transferred to the more electronegative element
either absorbed or released
always released
3
Mendeleev didn't list all elements in order of inc. atomic mass bc he grouped them with similar
colors
properties
densities
atomic numbers
4
Br belongs to Group 17. How many electrons does bromine have in its outermost energy level?
18
7
17
5
5
The number of valence electrons in Group 17 elements is
17
7
8
equal to the period
6
A negative ion is known as a(n)
ionic radius
cation
anion
valence electron
7
The most electronegative element is
H
Na
Br
F
8
In nature, the alkali metals occur as
complex ions
elements
compounds
gases
9
Identify the sublevels in a period that contains 32 elements.
s, f
s, p, d
s, p
s, p, d, f
10
Nitrogen's electron configuration is 1s
2
2s
2
2p
3
. To what group does nitrogen belong?
group 15
group 17
group 7
group 2
11
As each successive electron is removed, the ionization energy
remains the same
increases
decreases
12
Compared to the alkali metals, the alkaline-earth metals
are less dense
combine more readily with nonmetals
are less reactive
have lower melting points
13
Potassium and bromine belong to
period 1
group 4
period 4
group 1
14
The number of valence electrons in Group 14 elements is
4
8
7
equal to the period
15
In Group 2 elements, the valence electrons are in sublevel
f
d
p
s
16
In groups 13 through 18, valence electrons may be in sublevels
s and p
p and d
d and f
s and d
17
A ability of an atom in a chemical compound to attract electrons from another atom is called
ionization potential
electron affinity
electronegativitity
electron configuration
18
The idea of arranging elements according to their chemical & physical prop. is attributed to
Bohr
Moseley
Ramsay
Mendeleev
19
How much greater is Z of the 5th element in groups 1, 2, and 18 than the preceding element?
3
4
20
18
20
Across a period in the periodic table, atomic radii
gradually decrease
gradually increase
gradually decrease, then sharply increase
gradually increase, then sharply decrease
21
The electrons available to be lost, gained, or shared when atoms form compounds are called
electron clouds
valence electrons
d electrons
ions
22
The electron configuration of cesium, atomic number 55, is [Xe] 6s1. In what group is cesium?
group 8
group 15
group 6
group 1
23
Mendeleev predicted that the spaces in his periodic table represented
undiscovered elements
radioactive elements
isotopes
unstable elements
24
Elements to the right side of the periodic table (p-block) have properties most associated with
nonmetals
gases
metals
metalloids
25
The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Al is in Period
3
6
13
2
26
Because the first energy level contains only the 1s sublevel, the # elements in this period is
1
8
2
4
27
How many elements are in a period in which only the s and p sublevels are filled?
2
18
32
8
28
The most characteristic property of the noble gases is that they
have low boiling points
are radioactive
are gases at ordinary temperatures
are largely unreactive
29
The person whose work led to a periodic table based on increasing atomic number was
Moseley
Cannizzaro
Rutherford
Mendeleev
30
The periodic law states that the properties of elements are functions of their atomic
masses
radii
numbers
charges
31
As the atomic number of the metals of Group 1 increases, the ionic radius
remains the same
increases
decreases
cannot be determined
32
What are the elements with atomic numbers from 58 to 71 called?
the actinides
the lanthanides
the alkali metals
the noble gases
33
When determining the size of an atom, the radius of an atom is
equal to the distance between nuclei
one-half the distance between nuclei
one-fourth the distance between nuclei
twice the distance between nuclei
34
The discovery of what elements added a new column to Mendeleev's periodic table?
transition elements
metalloids
radioactive elements
noble gases
35
The electron configurations of the noble gases from Ne to Rn make these elements part of the
p block
s block
f block
d block
36
What are the radioactive elements with atomic numbers from 90 to 103 called
the rare-earth elements
the lanthanides
the noble gases
the actinides
37
A positive ion is known as a(n)
ionic radius
anion
cation
valence electron
38
Hydrogen is placed separately from other elements in the table because it
has atomic number one
does not exist as a free element in nature
is a gas
has many unique properties
39
Elements in which the d-sublevel is being filled have the properties of
metals
gases
metalloids
nonmetals
40
When an electron is acquired by a neutral atom, the energy change is called
electron configuration
ionization energy
electron affinity
electronegativitity
