Honors Chemistry Final Review 2013
TOPICS
Stoichiometry with LR
Nuclear
Quantum
PT Trends
Solubility
Molecular Geometry
Organic
Thermochemistry
Gas Laws
1.
Two isotopes of the same element will have the same number of
a. neutrons and electrons
c. neutrons and nucleons
b. protons and nucleons
d. protons and electrons
2.
Which sample contains the same number of atoms as 24 grams of carbon?
a. 80. g Ar
b. 10. g He
c. 24 g Mg
d. 4.0 g He
3.
A Ca+2 ion differs from a Ca atom in that the Ca+2 ion has
a. more protons
b. fewer protons
c. more electrons
d. fewer electrons
3.
At the end of 12 days, ¼ of an original sample of a radioactive element remains. What is the
half-life of the element.
a. 24 days
b. 48 days
c. 3 days
d. 6 days
4.
What is the total number of nucleons (protons and neutrons) in an atom of selenium ( atomic
number = 34, atomic mass = 79)
a. 34
b. 45
c. 79
d. 113
5.
As a substance changes from a liquid to a gas, the average distance between the molecules
a. decreases
b. increases
c. remains the same
6.
Which particle has a mass of approximately 1 mass unit and a unit positive charge?
a. neutron
b. proton
c. electron
d. alpha particle
7.
When a radioactive nucleus emits a beta particle (a negatively charged particle) , the atom’s
a. mass number is increased by 1
c. atomic number is increased by 1
b. mass number is decreased by 1
d. atomic number is decreases by 1
8.
The structure of an alpha particle is the same as a
a. lithium atom
b. neon atom
c. hydrogen nucleus
d. helium nucleus
9. In the Bohr model of the hydrogen atom, what is the value of n in the ground state?
10.
11.
Give the total capacity for electrons of the principal energy level for which
a . n= 1
b. n=2
c. n=3
d. n=4
Which has higher energy, an electron in the
a. 1st or 2nd energy level?
b. 1s or 2s sublevel?
c. 2s or 2p sublevel?
d. 3d or 4d sublevel?
e. n=5
12.
What is the highest energy sublevel in the principal energy level for which n is
a. 1
b. 2
c. 3
d. 4
13.
What is the capacity for electrons in each of the following sublevels?
a. s
b. p
c. d
d. f
14.
What is the total capacity for electrons in
a. an orbital
b. an s sublevel
d. the 1st principal energy level
15.
c. a p orbital
e. the 3rd principal energy level?
Which of the following sublevels do not exist?
a . 2p
b. 1p
c. 2d
d. 3d
e. 3f
16.
Arrange the following sublevels in order of increasing energy:
1s, 3p, 2s, 2p, 3s
17.
In the third principal energy level, what is the total electron capacity?
How many different sublevels are in this level?
List them in order of increasing energy.
18.
How many orbitals are there in the following sublevels?
a. s
b. p
c. d
d. f
19.
What is the total number of orbitals in the principal energy level for which n is:
a. 1
b. 2
c. 3
d. 4
20.
Give the outer electron configuration of the elements in the following groups of the Periodic
Table:
a. 3
b. 5
c. 17
d. 18
e. 13
f. 8
Example: Group 2 ns2
21.
Which group in the Periodic Table has the outer configuration:
a. ns2
b. ns2np2
c ns2np5
22.
Give the total number of outermost level electrons (valence electrons) of an element in Group
a. 1
b. 13
c. 14
d. 16
e. 17
23.
In what group of the Periodic Table do all the elements have:
a. 2 valence electrons
b. 5 valence electrons
c. 6 valence electrons?
Write the electron configuration of
a. B
b. Ne
c. Al
e. Ca
24.
d. Cl
25.
Identify the elements which have the following outer electron configuration:
a. 3s23p3
b. 4s1
c. 6s26p5
d. 5s25p4
26.
Determine the atomic number of the element in which there is (are):
a. a single 2s electron
b. two 2p electrons
c. five 3d and two 4s electrons
d. an equal number of 4s and 3d electrons
27..
In a certain atom, the first and second principal energy levels are completely filled, as is the 3s
sublevel. There are three electrons in the 3p sublevel.
a. How many electrons are there in the atom?
b. Give the electron configuration of the atom.
c. What is the element’s symbol?
28.
Give the number of electrons in each of the 3p orbitals in each of the following elements:
a. Al
b. Br
c. Ca
d. O
e. Ar
f. T i
g. Fe
h. Sb
I. Ge
j. C
PERIODIC TABLE:
29.
How many groups are in the periodic table? ___________ How many periods? ____________
30.
Define atomic number _________________ What information does it convey? _____________
31.
What is mass number ? __________________________________________________________
32.
What number, other than atomic number is represented for every element in the periodic
table?____
33.
How many elements are in period 1_____________? 2? __________ 3? ___________ 4? _____
34.
In which group are the noble gases found? __________________________________
35.
Why are the noble gases special? ___________________________________________________
36.
In how many groups are the s-sublevels filled? ________ p-sublevels filled? _______________
d-sublevels filled? ________________ f-sublevels filled? ____________________________
37.
What block in the periodic table contains the transition elements? _______
The rare earth elements (lanthanoids and actinoids)? _____________
38.
What do the elements in a group have in common? _____________________________________
39.
What is an ion? _________________________________________________________________
40.
How does an atom form an ion?____________________________________________________
41.
How does an atom form a cation?___________________________________________________
42.
How does and atom form an anion?_________________________________________________
43.
Which groups form cations? _________________________________
44.
Which groups form anions? _________________________________
45.
Draw the outermost energy electron diagrams (Lewis Structures) for elements in groups 1, 2, 13,
17, and 18.
46.
What is the charge on the ions formed by elements in groups 1, 2, 17, and 18. ( Indicate + or - as
well as magnitude of the charge)
47.
For each of the following pairs, use the periodic table to select the atom that is larger in radius.
a. Rb, Sr
b. Cl, I
c. Na, Rb
d. Mg, Be
e. S, P
f. Ac, U
g. B, Al
h. Au, Ba
48.
ions?
How many electrons are lost or gained to complete the outer octet and produce the following
a. K+1
f. Br1-
b. O-2
g. Ca2+
c. Ga+3
h. Sc3+
d. P3-
e. Sn4+
49.
Which atom in each of the following pairs would have the lower first ionization energy?
a. N, O
b. Te, Sn
c. Ne, F
d. C, Ge
e. Br, I
f. Mg, Ca
g. I, Sb
h. Al, N
I. F, S
50.
Within a group, do the radii of atoms increase or decrease as the atomic number increases?
51.
Does the radii of atoms within a period increase or decrease as the atomic number increases?
52.
In each of the following pairs of atoms, pick the one that is larger.
a. Mg, Na
b. K, Ca
c. Al, B
e. F, N
f. Ne, Ar
53.
d. Br, Cl
In a group, will the ionization energy tend to increase or decrease with increasing atomic number?
54.
In a period, will the ionization energy tend to increase or decrease with increasing atomic
number?
PROPERTIES OF METALS AND NONMETALS
55.
Compare the following in terms of:
METALS
Ionization Energy
Electronegativity
Luster
Deformability(Malleability, Ductittility)
Conductivity of Heat
Conductivity of Electricity
Phase at Room Temperature
Ion Formation (Positive or Negative)
Number of Electrons in outermost Energy Level
NONMETALS
PROBLEMS
1.
Nitrogen-13 emits beta radiation and decays to carbon-13 with a half-life of 10 minutes. Assume
a starting mass of 2.0 g of nitrogen-13. How many grams of that isotope will remain after four
half lives?
2.
A patient is administered 20 mg of iodine-131. How much of this isotope will remain in the body
after 40 days if the half-life of iodine-131 is 8 days?
3.
Complete and balance the equations for the following nuclear reactions:
a.
27
13
b.
214
83
Al +
2
4
4
2 He
Bi →
c.
27
14 Si
d.
66
29
e.
9
4
→
0
1 e
66
30
Cu →
Be +
He →
4
2
30
14
Si + ?
+ ?
+ ?
Zn + ?
He →
12
6
C + ?
4. Devise a way to separate sand from a mixture of charcoal, sand, sugar, and water.
5. How are the three isotopes of hydrogen alike? How are they different?
6. How do the terms group and period relate to the periodic table?
7. How is a representative (main group) element’s outer electron configuration related to its position in
the periodic table?
8. Explain why atoms form chemical bonds and describe the difference between an ionic and covalent
bond.
9. Why is the possible to bend metals but not ionic crystals?
10. Explain briefly why metals are good conductors of electricity.
11
12.
13.
a) What is the % of oxygen in NaClO3
b) What is the % of N in Ca(NO3)2
What is the molecular formula of :
(a) Molar mass 160
(b) molar mass 229
Fe 70.0 %
P = 26.6 %
O 30.0%
Mg = 31.4%
O = 42.0 %
(c) molar mass 146
Cd = 22.4 g
O = 6.4 g
H = 0.4 g
(a) 5.0 L of SO2(g) at 27 ºC and 760 mm Hg is what volume at 23 ºC and 1520 mm Hg?
(b) What pressure is needed to hold 22.0 g of CO2(g) in 4.0 L at 27 ºC?
( c) 3.4 g NH3 has what volume at STP?
(d) What is the comparative rate of diffusion between CO2 and O2?
14.
Note: balance the equation before proceeding to solve the problems.
(a) How many moles of O2 are needed to burn 112 g of CO into CO2?
CO + O2 → CO2
(b) How many grams of HCl will be produced from 7.1 g of Cl2?
C10H16 + Cl2 → C + HCl
(c) How many liters of NH3 are needed to make 72 g H2O at STP?
NH3 + O2 → NO + H2O
(d) How many liters of O2 are needed to burn 40.0 L of C2H6(g) at STP?
(e) How many grams of N2 can be made from 3.4 g NH3 and 6.4 g O2?
4NH3(g) + O2(g) → 2N2(g) + 6H2O(l)
15. (a) How many calories are needed to raise the temperature of 25 g of H2O from 20.0 ºC to 65.0 ºC?
(b) 0.50 g of C2H6 burns in a calorimeter. 200.0 g of water changes from 20.0 ºC to 57.0 ºC. What
is the molar heat of combustion?
( c) 10.0 g of ice is placed in H2O. How many calories of heat will it gain to become 10.0 g of
H2O(l) at 0.0 ºC?
16. (a) What is the molarity of 10.0 g NaOH in 250 ml solution?
(b) How many grams of AgNO3 are needed to make 6.0 L of 2.0 M solution?
17.
0.001 M HCl = ? pH
.0001 M HCl = ? pH
0.01 M NaOH = ? pH
0.1 M NaOH = ? pH
pH = 1 [H+] = ?
pH = 10 [OH-] = ?