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Trends of the Periodic Table
Trends of the Periodic Table
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Chemistry Chapter 14
Flashcards
48 cards
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Practice quiz
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Questions
48
Answers
1
Another name for the Group 1A elements is the ___.
noble gases
alkaline earth metals
alkali metals
halogens
2
What element in the second period has the largest atomic radius?
beryllium
potassium
carbon
neon
3
The atomic number of an element is the total number of which particles in the nucleus?
protons and electrons
protons
electrons
neutrons
4
Which family of elements is characterized by an s
2
p
5
configuration?
Group 7A
Group 7B
Group 5A
Group 5B
5
Which of the following groupings contains only representative elements?
Rb, F, In
Al, Mg, Sc
Cu, Co, Cd
Ni, Fe, Zn
6
What is another name for the representative elements?
transition metals
Group A elements
Group B elements
Group C elements
7
Which subatomic particle plays the greatest part in determining the properties of an element?
none of the above
proton
electron
neutron
8
Which of the folowing is a transition metal?
zirconium
tellurium
tin
cesium
9
What causes the shielding effect to remain constant across a period?
The atomic radius increases.
The charge on the nucleus is constant.
Electrons are added to different principal energy levels.
Electrons are added to the same principal energy level.
10
How does the atomic radius change from left to right across a period in the periodic table?
It tends to increase.
It first decreases, then increases.
It tends to decrease.
It first increases, then decreases.
11
What is the charge of a cation?
depends on the size of the nucleus
no charge
positive
negative
12
Which of the followng is true about the electron configurations of the noble gases?
The electron with the highest energy in the d sublevle.
The highest occupied s and p sublevels are partially filled.
The highest occupied s and p sublevels are completely filled.
The electrons with the highest energy are in the f sublevle.
13
What is the element with the highest electronegativity?
calcium
fluorine
cesium
helium
14
Elements that are characterized by the filling of d orbitals are classified as
transitional metals
group 1A and 2A
groups 3A through 8A
inner transitional metals
15
Which of the following is true about cations?
anions form when an atom loses protons
cations form when an atom loses electrons
cations form when an atom gains electrons
anions form when an atom gains protons
16
_______ measures the ability of a bonded atom to attract electrons to itself.
Ionization energy
Electronegativity
Magnetism
Nuclear energy
17
Which of the following increases with increasing atomic number in Group 2A?
shielding effect
ionization energy
malleability
electronegativity
18
Which of the following elements is in the same period as phosphorus?
carbon
oxygen
chlorine
nitrogen
19
Why is the second ionization energy greater than the first ionization energy?
The size of the anions decreases across a period.
The nuclear attraction from the protons in the nucleus decreases.
The size of atoms increases down a group.
It is more difficult to remove a second electron from an atom.
20
Which statement is true about electronegativity?
It generally increases from left to right.
It is the ability of an anion to attract another anion.
It generally increases as you move from top to bottom.
It generally is higher for metals than nonmetals.
21
Which of the following has the smallest atomic radius?
strontium
rubidium
cesium
barium
22
Each period in the periodic table corresponds to _____.
an orbital
an energy sublevel
a suborbital
a principal energy level
23
Which of the following factors contribute to the increase in atomic size within a group as the atomic number increases?
fewer electrons in the highest occupied energy level
an increase in the number of protons
an increase in the size of the nucleus
more shielding of the electrons by the highest occupied energy level
24
Which of the following is a metalloid?
As
Se
Al
Sn
25
Which of the following is true about the electron configurations of the representative elements?
The electrons with the highest energy are in an f sublevel.
The highest s and p sublevels are completely filled.
The electrons with the highest energy are in a d sublevel.
The highest occupied s and p sublevels are partially filled.
26
For Group 2A metals, which electron is the most difficult to remove?
All the electrons are equally difficult to remove.
the third
the first
the second
27
Atomic size generally _______.
increases as you move from left to right across a period
decreases as you move from top to bottom
remains constant within a period
decreases as you move from left to right
28
Which of the following statements correctly compares the relative size of an ion to its neutral atom?
The radius of an anion is identical to the radius of its neutral atom.
The radius of a cation is greater than the radius of its neutral atom.
The radius of an anion is greater than the radius of its neutral atom.
The radius of a cation is identical to the radius of its neutral atom.
29
Which of the following factors contribute to the decrease in ionization energy within a group from top to bottom?
fewer electrons in the highest occupied energy level
increase in number of protons
increase in atomic size
increase in size of the nucleus
30
Of the following elements, which one has the largest first ionization energy?
Ga
Al
Ge
Si
31
In which of the following sets are the charges given correctly for all the ions?
N-, O 2-, F 3-
K+, Sr 2-, O 2-
Na +, Mg 2+, Al 3+
Rb -, Ba 2-, P 3+
32
Which of the followng elements has the lowest electronegativity?
Si
Br
Na
Cl
33
Which elements are described as those containing electrons in the outermost s and nearby f sublevels?
halogens
transition metals
noble gases
inner transition metals
34
What are the Group 2A and 6A examples of?
representative elements
nonmetallic elements
noble gases
transition elements
35
The modern periodic table is arranged in order of increasing atomic _____.
charge
mass
number
radius
36
What is another name for the transition metals?
Group C elements
noble gases
Group A elements
Group B elements
37
What is the energy required to remove an electron from an atom in the gaseous state called?
nuclear energy
shielding energy
ionization energy
electronegative energy
38
Which of the following electron configurations is most likely to result in an element the is relatively inactive?
a filled energy level
one empty and one filled energy sublevel
a half-filled energy sublevel
a filled highest occupied principal energy level
39
Of the following elements, which one has the smallest first ionization energy?
Rb
Ca
Sr
K
40
Which of the following elements is a representative element?
Mo
Pt
Pu
Si
41
Which of the following categories includes the majority of the elements?
metalloids
liquids
metals
nonmetals
42
How does atomic radius change from top to bottom in a group in the periodic table?
It tends to increase
It tends to decrease
It first increases, then decreases
It first decreases, then increases
43
Which of the following elements is a nonmetal?
Pt
V
Na
Se
44
Which element has the lowest electronegativity value?
calcium
francium
fluorine
helium
45
AS you move from left to right aross the second period of the periodic table ___.
electronegativity decreases
atomic mass decreases
atomic radii increase
ionization energy increases
46
Which of the following factros contributes to the increase in ionization energy from left to right across a period?
an increase in the number of protons
fewer electrons in the highest occupied energy level
an increase in the size of the nucleus
an increase in the shielding effect
47
What element ends with electron configuration sublevel of 3p
4
?
silicon
sufur
selenium
germanium
48
Compared with the electronegativities of the elements on the left side of a period, the elements on the right side ___
tend to be higher
tend to be unpredictable
tend to be the same
tend to be lower
