Accel Chemistry 2nd quarter review J
Name: ______
Date: ______
Write the electron configurations for the following elements.
1. O: 1s22s22p4
2. Ca:1s22s22p63s23p64s2
3. Cu: 1s22s22p63s23p64s23d9
4. Sn: 1s22s22p63s23p64s23d104p65s24d105p2
5. Rn: 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p6
Name the groups of the periodic table.
1. __Alkali Metals______
2. ___Alkaline Earth Metals______
17. __Halogens______
18. ___Noble Gases______
D-Block: ___Transition Metals______
4f: __Lanthanide______
5f: ___Actinide______
Circle the element that fits the statement
Li Si S metal
N P As smallest ionization energy
K Ca Sc largest atomic mass
S Cl Ar member of the halogen family
Al Si P greatest electron affinity
Ga Al Si largest atomic radius
V Nb Ta largest atomic number
Te I Xe member of noble gases
Si Ge Sn 4 energy levels
Li Be B member of alkali metals
As Se Br 6 valence electrons
H Li Na nonmetal
Hg Tl Pb member of transition metals
Na Mg Al electron distribution ending in s2p1
Pb Bi Po metalloid
B C N gas at room temperature
Ca Sc Ti electron distribution ending in s2d2
Trend Review
- Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.
O, C, Al, K
- Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum.
Ne, Al, S, O
- Why does fluorine have a higher ionization energy than iodine?
Effective nuclear charge is higher – the + charge of the nucleus is stronger for F than I – the nucleus of F is able to attract electrons to it better than I.
- Why do elements in the same family generally have similar properties?
They have the same number of valence electrons.
- Indicate whether the following properties increase or decrease from left to right across the periodic table.
- atomic radius (excluding noble gases) Decreases
- first ionization energy Increases
- electronegativity Increases
- What trend in atomic radius occurs down a group on the periodic table? What causes this trend?
It increases because of electron shielding – the core electrons block the valence electrons from feeling the pull of the + nucleus and it allows the valence electrons to get further and further from the nucleus thus expanding the size of the atom.
- What trend in ionization energy occurs across a period on the periodic table? What causes this trend?
It increases because of effective nuclear charge – the atoms are more able to remove an electron from an atom because the nucleus is gaining + protons and the atom is getting smaller. As you move across the table, the atoms want to gain electrons more and more (until you get to the noble gases).
- Circle the atom in each pair that has the largest atomic radius.
Accel Chemistry 2nd quarter review J
- Al or B
- Na or Al
- S or O
- O or F
- Br or Cl
- Mg or Ca
Accel Chemistry 2nd quarter review J
Accel Chemistry 2nd quarter review J
- Circle the atom in each pair that has the greater ionization energy.
Accel Chemistry 2nd quarter review J
- Li or Be
- Ca or Ba
- Na or K
- P or Ar
- Cl or Si
- Li or K
Accel Chemistry 2nd quarter review J
- Define electronegativity.
Electronegativity is the ability of a bonded atom (one that is bonded to something else already) to attract electrons to it.
- Circle the atom in each pair that has the greater electronegativity.
Accel Chemistry 2nd quarter review J
- Ca or Ga
- Br or As
- Li or O
- Ba or Sr
- Cl or S
- O or S
Accel Chemistry 2nd quarter review J
Bonding Review
12. List three differences between ionic and covalent compounds:
Ionic bonds transfer electrons and covalent bonds share electrons.
Ionic bonds are stronger.
Ionic bonds have a metal bonded to a nonmetal (they are far apart on the PT) and covalent bonds are between 2 nonmetals (close together on the PT).
13. Explain why ionic compounds are formed when a metal bonds with a nonmetal but covalent compounds are formed when two nonmetals bond.
The metal and nonmetal in an ionic bond have a large electronegativity difference so 1 atom takes the other atoms electrons. The 2 nonmetals in a covalent bond doesn’t have a large electronegativity difference so 1 atom doesn’t pull the other atom’s electrons off of it – they still share the electron.
14. What does electronegativity have to do with bond polarity?
Electronegativity difference (when sharing and e-) results in 1 atom having a better ability to pull electrons to it which make the electrons around it more than the other. This creates an electron density difference in the molecule which makes one side slightly positive and the other side slightly negative.
15. Explain how hydrogen bonding takes place.
The H that is part of a very electronegative bond (F, O, N) ends up with a slight positive charge and is attracted to another molecule’s F, N, or O atom since it is slightly positive. The hydrogen bonding happens between two different molecules.
16. Why is the bond length of nitrogen much shorter than the bond length of chlorine?
The length of a nitrogen bond is shorter than the length of a chlorine bond because the nitrogen bond is a triple bond and the chlorine bond is a single bond. Triple bonds are shorter than single bonds (the pi bonds shrink the distance between the atoms).
Draw the Lewis Structures for the following.
Accel Chemistry 2nd quarter review J
1. O
.
:O:
.
2. CH4
H
H-C-H
H
3. NI3
..
I-N-I
I
4. CS2
.. ..
:S=C=S:
10. C2H2
10. C2H2
11. OF2
......
:F-O-F:
......
12. CH3OH
H ..
H-C-O-H
H ..
13. NH4+
H +
H-N-H
Accel Chemistry 2nd quarter review J
5. NO2-
......
:O-N=O:
..
6. P2H4
.. ..
H-P-P-H
H H
7. SHF
.. ..
H-S-F:
.. ..
8. CF2S
.. ..
:F-C=S:
.. : F:
..
9. SCN-
..
:S-C=N:
..
H
14. CH3COO-
..
H :O: ..
H-C-C=O:
H
15. CN-
:C=N:
16. CO32-
2
Accel Chemistry 2nd quarter review J
Conversions
Accel Chemistry 2nd quarter review J
1. How many moles of silver are in 4.529 x 1017 atoms of silver?
4.529 X 1017 atoms 1 mole = 7.52 x 10-7 mol Ag
6.022 x 1023 atoms
2. How many atoms are in 3.731 moles of silver?
3.731 mol Ag 6.022 x 1023 atoms = 2.247 x 1024 atoms
1 mol Ag
3. Convert 5.1 moles of chlorine to grams of chlorine.
5.1 mol Cl 35.453 g Cl = 180.810 g Cl
1 mol Cl
4. Convert 0.94 moles of rubidium to grams of rubidium.
0.94 mol Rb 85.468 g Rb = 80.340 g Rb
1 mol Rb
5. Convert 150 grams of rubidium to atoms of rubidium.
150 g 1 mol 6.022 x 1023 atoms = 1.057 x 1024 atoms
85.468 g 1 mol
6. How many grams are there in 6.4 x 1023 atoms of osmium?
6.4 x 1023 atoms Os 1 mol 190.23g = 202.171 g Os
6.022 x 1023 atoms 1 mol
7. What is the frequency of light if its wavelength is 5.4 X 10-7 m?
3.0 x 108 m / s = 5.556 x 1014 Hz c=λν v=c/λ
5.4 x 10-7 m
8. While doing an experiment in light, Sara finds that the light emitted by his sample has a frequency of 4.62 X 1014 Hz. What is the wavelength of the light?
Accel Chemistry 2nd quarter review J
3.0 x 108 m/s = 6.49 x 10-7 m
4.62 x 1014 Hz