Download 1. Which of the following is the most important - Hatboro

1.
Which of the following is the most important factor in determining the properties of an
element?
a. Atomic mass
b. Atomic radius
c. Periodic table position
d. Electron configuration
2.
Similar properties for chemical elements recur at certain intervals of atomic number.
Therefore, these properties are referred to as
a. Intensive
b. Periodic
c. Extensive
d. Intermittent
As the principle quantum number increases, the size of the electron cloud
a. Increases
b. Decreases
c. Remains constant
d. Varies at random
As you look across a period from left to right in the periodic table, the size of the atoms
a. Increases
b. Decreases
c. Remains constant
d. Varies at random
In which of the following pairs of particles does the second particle listed have the
smaller radius?
a. Ni, K
b. Na, Cs
c. Cl, Cld. Li, Li+
3.
4.
5.
6.
Which of the following electron configurations represents the particle that is most stable
chemically?
a. 1s2 2s2 2p6 3s2 3p5
b. 1s2 2s2 2p3
c. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d5
7.
What is the likeliest oxidation number of an element located in Period 3 and Group 16?
a. +2
b. +3
c. -3
d. -2
8. The amount of energy required to remove the most loosely held electron from an atom
is the
a. First ionization energy
b. Energy of formation
c. Bonding energy
d. Activation energy
9. Phosphorus has a first ionization energy of 1011.8 kilojoules per mole. Which of the
following elements has a first ionization energy less than that of phosphorus?
a. F
b. Ga
c. N
d. Cl
10. Which of the following is not a factor that affects ionization energy?
a. Nuclear charge
b. Shielding effect
c. Electron spin
d. Atomic radius
11. As you move through a period from metals to nonmetals, the first ionization energy
a. Increases
b. Decreases
c. Remains constant
d. Varies at random
12. For each subsequent electron removed from an atom, the ionization energy required
a. Increases
b. Decreases
c. Remains constant
d. Varies at random
13. A measure of the attraction of an atom for additional electrons is referred to as
a. Multiple ionization energies
b. Electronegativity
c. Electron affinity
d. Combining capacity
14. In general, as electron affinity increases, ionization energy
a. increases
b. decreases
c. remains constant
d. varies at random
15. As you move down through a group, electron affinity
a. Increases
b. Decreases
c. Remains constant
d. Varies at random
16. If two elements have similar chemical properties, you would expect them to have
a. Similar atomic radii
b. The same number of energy levels
c. The same number of outer electrons
d. Similar atomic masses
17. Which of the following has the greatest impact on the atomic radius as you move down
through a group?
a. Increased principle quantum number
b. Increased nuclear charge
c. Increased atomic mass
d. Decreased electron shielding effect
18. Which of the following describes the size of the elements’ ions as you move from left to
right across the periodic table?
a. Increases
b. Decreases
c. Remains constant
d. Decreases, then increases
19. In which of the following pairs of particles does the second particle listed have the
larger radius?
a. Rb, Y
b. Br, F
c. S-2, S
d. Ga-3, As+3
20. Elements in the same group or family in the periodic table have which of the following
characteristics in common?
a. The principle quantum number of the outer energy level
b. The number of isotopes that exist
c. The atomic radius
d. The number of electrons in the outer energy level
21. Which of the following occurs when an element in Group 2 attains a stable electron
configuration?
a. It gains 2 electrons
b. It loses 2 electrons
c. It gains 6 electrons
d. It gains 8 electrons
22. What is the likeliest oxidation number of an element in Period 4 and Group 13?
a. +3
b. -3
c. _4
d. -1
23. The first ionization energy of Ca is 589.9 kilojoules per mole. Which of the following
elements has a first ionization energy greater than that of Ca?
a. K
b. Rb
c. Sr
d. Mg
24. If an element has a high ionization energy, its electron affinity is
a. High
b. Low
c. Zero
d. Completely unpredictable
25. The electron configuration of K+ is most similar to that of
a. K
b. Na+
c. Ar
d. Ca+2
26. The radii of the atoms become smaller from sodium to chlorine across period 3. This
decrease is primarily a result of
a. The shielding effect
b. Increased nuclear charge
c. Increased number of electrons
d. Decreased metallic character
Look at a periodic table to answer the following questions:
1.
2.
3.
4.
5.
6.
7.
What is the name of group 1?
What is the name of group 2?
What is the name of group 17?
What is the name of group 18?
What is the name for the d block?
What is the name for the s & p block?
What is the name for the 2 periods at the bottom of the periodic table?
Answer the following questions with these terms:
Noble gases
Transition metals
Halogens
Alkali metals
Alkaline-earth metals
8. The _____________________ have a single electron in the highest energy level?
9. The _____________________ achieve the electron configurations of noble gases by
losing two electrons.
10. The _____________________ vary in the number of electrons in the highest energy
level.
11. The _____________________ achieve the electron configurations of noble gases by
gaining one electron.
12. The _____________________ have full s and p orbitals in the highest occupied energy
levels.
13. The _____________________ are stable and unreactive.
14. The _____________________ are highly reactive and readily form salts with metals.
15. The _____________________ are metals that are more reactive than the transition
elements but less reactive than the alkali metals.
3
Li
Lithium
6.94
11
Na
Sodium
22.989
4
Be
Beryllium
9.0121
12
Mg
Magnesium
24.305
16. Which element will react more readily with
chlorine: sodium or magnesium? Why?
17. Which element is more like lithium in terms of
properties: sodium or beryllium? Why?
18. Which element has more electrons in its highest
occupied energy level: sodium or magnesium?
19. Which element has a lower melting point: lithium or beryllium?
20. Which element is closer to achieving noble gas configuration: magnesium or lithium?
21. Which element reacts more readily with fluorine: lithium or beryllium? Why?
For each choice of words, circle the one that best completes the sentence.
1. The shielding effect increases with increasing atomic number within a (period, group).
2. In any (period, group), the number of electrons between the nucleus and the outer energy
level is the same.
3. Within a group, the nucleus has a stronger ability to pull on the outermost electrons in
elements of (high, low) atomic number.
4. The more (positive, negative) the value of electron affinity is, the more easily the atom
can take on an extra electron.
5. From left to right across a period, electron affinity values become more (positive,
negative).
6. The halogens have the (most, least) negative electron affinity values.
7. The (electronegativity, electron affinity) of an atom is the tendency of an atom to attract
electrons to itself when it is chemically combined with another element.
8. The (noble gases, halogens) are the most electronegative group.
Use the following choices:
a. increases
b. decreases
c. remains constant
d. there is no pattern
9. Moving from top to bottom in a group, atomic radius tends to _____________.
10. Moving from top to bottom in a group, shielding effect tends to _____________.
11. Moving from top to bottom in a group, electronegativity tends to _____________.
12. Moving from top to bottom in a group, electron affinity tends to _____________.
13. Moving from top to bottom in a group, ionization energy tends to _____________.
14. Moving from left to right across a period, atomic radius tends to _____________.
15. Moving from left to right across a period, shielding effect tends to _____________.
16. Moving from left to right across a period, electronegativity tends to _____________.
17. Moving from left to right across a period, electron affinity tends to _____________.
18. Moving from left to right across a period, ionization energy tends to _____________.
19. Which atom has the more negative value for electron affinity, sodium or chlorine?
20. Which atom is more electronegative, fluorine or lithium?
21. Which atom has a greater ionization energy, nitrogen or bismuth?
22. Which atom exerts a stronger pull on its outermost electrons: calcium or arsenic?
23. Which atom has a larger atomic radius, fluorine or barium?
24. Which atom has a greater nuclear charge, boron or selenium?