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Name ______________________________
Chemistry 4-12
Date _________________ Period ____
Review Guide for Periodic Trends
1) A period is a ________________________ _______________________ on the Periodic Table.
(vertical, horizontal)
(row, column)
2) A group is a ________________________ _______________________ on the Periodic Table.
(vertical, horizontal)
(row, column)
ATOMIC RADIUS
3) Atomic radius is the distance between the ___________________________ and the
______________________________________________________________________.
4) Atomic radius generally _____________________ as you move down a group. Valence electrons
(increases, decreases)
occupy _________________________ principal energy levels as you move down a group. As a result, the
(lower, higher)
electrons are ___________________________ from the nucleus. Thus, the electrons are
(closer, further)
________________________ held by the nucleus and the atomic radius is ___________________.
(tightly, loosely)
(small, large)
5) Atomic radius generally ____________________ as you move left-to-right across a period. This
(Increases, decreases)
is because within a period, all electrons are being added to the _____________________ shell. But, at
(same, different)
the same time, protons are being added to the nucleus, making it ________________ positively charged.
(more, less)
Thus, the nucleus attracts the electrons more strongly, having the atom’s shell pull _____________ to the
(closer, farther)
nucleus. The valence electrons are held ___________________ towards the nucleus of the atom. As a
(closer, farther)
result, the atomic radius ____________________ left-to-right.
(increases, decreases)
Chemistry
4-12
IONIZATION ENERGY
6) Ionization energy is the amount of energy needed to _________________ an ________________
(remove, add)
(proton, electron)
from an atom. The smaller the ionization energy, the ______________ it is to remove an electron.
(easier, harder)
7) Ionization energy ____________________ as you go left-to-right on the Periodic Table.
(increases, decreases)
Elements on the left side of the Periodic Table have _______________ ionization energies, because they
(lower, higher)
have a greater willingness to ______________ electrons in effort to have a full valence shell (8 valence
(lose, gain)
electrons). Elements on the right side of the Periodic Table have ______________ ionization energies,
(lower, higher)
because their valence shell is already nearly filled.
8) As you move down a group, ionization energy generally ________________. This is because the
(increases, decreases)
number of principal energy shells ____________________ down a group and thus there is an
(increase, decrease)
____________________ distance between the valence electrons and nucleus, or a greater atomic radius.
(increased, decreased)
9) Group 18 (noble gases) possess very __________________ ionization energies because they have full
(high, low)
valence shells.
ALKALI METALS WITH WATER DEMO
10) In the video demo, we watched 3 different alkali metals (Li, Na, and K) react with ____________.
(oil, water)
The reactions were similar between all 3 metals because they are all found in the same _____________
(group, period)
and have the same number of _______________________________. Thus, all three metals have
(inner electrons, valence electrons)
similar chemical ___________________________. Lithium (Li) reacted the ___________________
(formulas, properties)
(most, least)
vigorously, while potassium (K) reacted the ___________________ vigorously.
(most, least)
11) As you go down Group 1, reactivity __________________.
(increases, decreases)
Chemistry 4-12
ELECTRONEGATIVITY
12) Electronegativity is the _______________________ of ________________________ by an atom.
(attraction, repulsion)
(protons, electrons)
The larger the electronegativity, the __________________ an atom attracts electrons.
(more, less)
13) As you move to the right across a period of elements, electronegativity ____________________.
(increases, decreases)
14) Most atoms prefer to fulfill the ______________ rule (having the valence shell comprise of 8
electrons). Elements on the left side of the Periodic Table have less than a half-full valence shell. Thus it is
easier (takes less energy) to lose electrons to create a full valence shell, rather than gain electrons. Thus
atoms on the left-side of the P.T. have a low attraction for electrons and have _____________
(low, high)
electronegativities.
15) Elements on the right side of the Periodic Table have more than a half-full valence shell, and it is
easier (takes less energy) to gain electrons to create a complete valence shell of 8 electrons. Thus atoms
on the right-side of the P.T. have a high attraction for electrons and have _____________________
(low, high)
electronegativities.
16) As you move down a group, electronegativity generally _________________. This is because the
(increases, decreases)
there is an ____________________ distance between the valence electrons and nucleus, or a greater
(increased, decreased)
atomic radius.
17) Group 18 (noble gases) possess a complete valence shell and do not usually attract electrons,
thus they _______________ have electronegativity values.
(do not, always)
Chemistry 4-12
Practice Questions
1. Of the following elements, which would have the
largest radius?
1)
2)
3)
4)
Lithium (Li)
Neon (Ne)
Boron (B)
Nitrogen (N)
(2) Period 2
(4) Group 1
11. Which elements have the most similar chemical
properties?
(1) K and Na
(3) K and Ca
(2) K and Cl
(4) K and S
2. Nitrogen has a larger atomic radius than Oxygen.
1) True
2) False
3. An atom with an atomic radius smaller than that of
Sulfur (S) is __________.
1) Oxygen (O)
2) Selenium (Se)
3) Calcium (Ca)
4) None of the above
4. Which two elements have the most similar chemical
properties?
(1) aluminum and barium
(3) chlorine and sulfur
(2) nickel and phosphorus (4) sodium and potassium
5. As the atoms of the metals of Group 1 in the ground
state are considered in order, from top to bottom, the
number of occupied principal energy levels
(1) decreases
(2) increases
(3) remains the same
6. Which element is in Group 2 and Period 7 of the
Periodic Table?
(1) magnesium
(3) radium
(2) manganese
(4) radon
7. Given the representation of chlorine above, which
circle would represent an atom of fluorine?
(1) b (2) c
(3) d (4) none of these
8. Which electron configurations represent the first two
elements in Group 17 of the Periodic Table?
(1) 2-1 and 2-2
(3) 2-7 and 2-8-7
(2) 2-2 and 2-3
(4) 2-8 and 2-8-7
9. Which is the electron configuration of an atom of
Period 3 element?
(1) 2-1
(3) 2-5
(2) 2-3
(4) 2-8-1
10. In which category of elements in the Periodic Table
do all of the atoms have valence electrons in the
second principal energy level (second shell)?
(1) Group 2
(3) the alkaline earth family
12. Using the diagrams above, which of these
elements would have the lowest ionization energy?
(1) a
(2) b
(3) c
(4) d
13. An atom of an element has 28 innermost electrons
and 7 outermost electrons. In which period of the
Periodic Table is this element located?
(1) 5
(3) 3
(2) 2
(4) 4
14. Atoms of elements in a group of the Periodic Table
have similar chemical properties. This similarity is
most closely related to the atoms’
(1) number of principal energy levels
(2) number of valence electrons
(3) atomic structure
(4) atomic masses
15. Which group below contains elements with the
greatest variation in chemical properties?
(1) Li, Be, B
(3) B, Al, Ga
(2) Li, Na, K
(4) Be, Mg, Ca
16. The chemical properties of the elements are
periodic functions of their atomic
(1) masses
(3) numbers
(2) weight
(4) radii
17. All of the atoms of the elements in Period 2 have
the same number of
(1) protons
(3) valence electrons
(2) neutrons
(4) occupied principal energy levels
Chemistry 4-12
18. Which is the electron configuration of an atom of a
Period 3 element?
(1) 2-1
(2) 2-3
(3) 2-5
(4) 2-8-5
19. In the ground state, atoms of the elements in
Group 15 of the Periodic Table all have the same
number of
(1) filled principal energy levels
(2) occupied principal energy levels
(3) neutrons in the nucleus
(4) electrons in the valence shell
20. Which of the Group 15 elements can lose an
electron most readily?
(1) N
(2) P
(3) As
(4) Bi
21. Which element is a member of the halogen family
(Group 17)?
(1) K
(2) B
(3) I
(4) S
22. In which group does each element have a total of
four electrons in the outermost principal energy level?
(1) 1
(2) 18
(3) 16
(4) 14
23. The electron dot structure for elements in Group
14 is
(1) X
(2) X
(3) X
(4) X
24. Elements in Group 18
(1) have 3 valence electrons in the last shell
(2) have 18 valence electrons in the first energy level
(3) have a complete outer shell
(4) have an incomplete outer shell
25. An atom of which of the following elements has the
smallest atomic radius?
(1) Li
(2) Be
(3) C
(4) F
26. Which of the following atoms has the largest
atomic radius?
(1) Na
(2) K
(3) Mg
(4) Ca
27. Which element has the highest ionization energy?
(1) sodium
(3) calcium
(2) aluminum
(4) phosphorus
28. Which element in Group 1 has the greatest
tendency to lose an electron?
(1) cesium
(3) potassium
(2) rubidium
(4) sodium
29. Which of the Group 15 elements can lose an
electron most readily?
(1) N
(2) P
(3) Sb
(4) Bi
30. Which first ionization energy is the most probable
for a very reactive metal?
(1) 380 kjoules/mol
(3) 1681 kjoules/mol
(2) 1086 kjoules/mol
(4) 2372 kjoules/mol
31. A nonmetal could have an electronegativity of
(1) 1.0
(2) 2.0
(3) 1.6
(4) 2.6
32. Of all the elements, the one with the highest
electronegativity is found in Period
(1) 1
(2) 2
(3) 3
(4) 4
33. A metal can have an electronegativity of
(1) 4.0
(2) 1.0
(3) 3.5
(4). 3.2
34. Which electronegativity is possible for a Group 1
metal?
(1) 1.0
(2) 2.0
(3) 3.0
(4) 4.0
35. According to Reference Table S, which of the
following elements has the smallest atomic radius?
(1) nickel
(3) calcium
(2) cobalt
(4) potassium
36. Which electron configuration represents the atom
with the largest atomic radius?
(1) 2-1
(2) 1
(3) 2-2
(4) 2-3
37. Which of the following elements has the largest
atomic radius?
(1) beryllium
(3) calcium
(2) magnesium
(4) strontium
38. Which element in Period 3 has the largest atomic
radius?
(1) Cl
(2) Al
(3) Na
(4) P
39. As the elements Li to F in Period 2 of the Periodic
Table are considered in succession, how do the relative
electronegativity and the atomic radius of each
successive element compare?
(1) the relative electronegativity decreases, and the
atomic radius decreases
(2) the relative electronegativity decreases, and the
atomic radius increases
(3) the relative electronegativity increases, and the
atomic radius decreases
(4) the relative electronegativity increases, and the
atomic radius increases
*40. Which element’s ionic radius is smaller than its
atomic radius?
(1) neon
(3) sodium
(2) nitrogen
(4) sulfur
*41. An ion of which element is smaller than its atom?
(1) F
(2) O
(3) Cl
(4) Na
*42. An ion of which element is larger than its atom?
(1) Al
(2) Br
(3) Ca
(4) Sr
*43. Which atom has a radius larger than the radius of
its ion?
(1) Cl
(2) Ca
(3) S
(4) Se
4-12 Review Guide
Answer Key
1. 1
2. 1
3. 1
4. 4
5. 2
6. 3
7. 1
8. 3
9. 4
10. 2
11. 1
12. 4
13. 4
14. 2
15. 1
16. 3
17. 4
18. 4
19. 4
20. 4
21. 3
22. 4
23. 4
24. 3
25. 4
26. 2
27. 4
28. 1
29. 4
30. 1
31. 4
32. 1
33. 1
34. 1
35. 1
36. 1
37. 4
38. 3
39. 3
40. 3
41. 4
42. 2
43. 2