Download Review Study Guide for the Final

Review Study Guide for the Final
Atomic Structure and Matter
1.
Define an element. The simplest form of matter that has it a unique set of properties, it
cannot be broken down into simpler substances by chemical means
2.
Define a compound. A substance that contains two or more elements chemically combined
in a fixed proportion
3.
Define matter.
4.
What is the atomic number?
5.
What is the atomic mass number of an element? Number of protons plus neutrons
6.
Where are electrons located? Outside the nucleus
7.
Where are protons located?
Inside the nucleus
8.
Where are neutrons located?
Inside the nucleus
9.
What is it called when you have more electrons than protons?
anion
10.
What is it called when you have more protons than electrons?
cation
11.
Do all elements have neutrons? No, Hydrogen does not normally have a neutron
12.
What are isotopes? Atoms of the same element that have the same atomic number but
different masses due to a different number of neutrons
Anything that has mass and occupies space
The number of protons
Periodic Table
13.
What is Periodic Law?
When elements are arrange in order of increasing atomic
number, there is a periodic repetition of their physical and chemical properties.
14.
Where are metals located at on the periodic table?
Left of the stair-step line
15.
Where are nonmetals located at on the periodic table?
Right of the stair-step line
16.
Where are semimetals located at on the periodic table?
On the stair-step line
17.
What is ionization energy? The amount of energy required to remove and electron from an
atom
18.
Elements in the same group have the same number of what?
19.
What are valance electrons?
20.
Where are the Alkali metals located?
21.
Where are the Alkaline earth metals located?
Valance electrons
The outermost electrons used for bonding
Column 1A
Column 2A
22.
Where are the Halogens located?
Column 17A also known as the second to last column
23.
Where are the Noble gases located?
Column 18A also known as the last column
Conservation of Mass and Stoichiometry
24.
What is a mole?
The amount of a substance that contains 6.02 x 1023 representative
particle of that substance
25.
What element is used to set the mass scale?
26.
What is Avogadro’s number? 6.02 x 1023
Carbon-12
Chemical Bonds
27.
Are electrons shared or transferred in an ionic bond?
Transferred
28.
Are electrons shared or transferred in a covalent bond?
Shared
Draw the Lewis Dot diagram for the following:
Br
.Br :
:
a.
:
29.
He
c.
Ar
He :
:
b.
:
: Ar :
30.
Combine the following ions
a.
Na+
CO32-
Na2CO3
b.
Sr2+
N3-
Sr3N2
c.
Al3+
Cl-
AlCl3
d.
Ca2+
OH-
Ca(OH)2
e.
Mg2+
PO43-
Mg3(PO4)2
f.
Mg2+
I-
MgI2
31.
Balance the following reactions:
a.
4Al +
3O2
→
b.
8Mg(s) + S8
→
8MgS
c.
3Ca +
N2
→
2Al2O3
Ca3N2
Solutions
32.
Define the following terms
A. Solution a homogeneous mixture involving two or more pure substances.
B. Solute substance dissolved in the solution.
C. Solvent the substance in which the solute is dissolved
33.
What is the molarity of HCl when 18.00 g of HCl (g) is added to water yielding a total
combined volume of 3.50L?
18.00g x
1 mole HCl
= 0.4938 moles
36.45g
0.4938 moles
3.50 L
34.
0.141 M
To what volume, in liters, must you dilute a solution containing 4 liters of 0.100 M of
Ca(OH)2 to obtain a 0.00100 M solution as calcium hydroxide (Ca(OH)2)?
(0.100M)(4L)
=
(0.00100M)(V2)
V2
35.
=
=
400L
How many grams of KMnO4 must be added to make 500 mL of 0.25M potassium
permanganate solution?
500mL x
1L
= 0.500L
1000mL
0.500L x
0.125 moles
0.25 moles
L
x
158.04g
mole
=
0.125 moles
=
19.755g
Reaction Rates and Equilibrium
36.
What is a catalyst?
the reaction.
A catalyst works by lowering the activation energy, this then speeds up
37.
Draw a reaction diagram for an endothermic reaction and for an exothermic reaction. Label
the products and the reactants.
Activation Energy
Activation Energy
Endothermic
Exothermic
Reactants
Products
Products
38.
Reactants
Predict how the following would change the direction of the given the following exothermic
reaction at equilibrium. Briefly support your answer. Will it “shift to the left or shift to the
right.”
N2 + 3H2 Æ 2 NH3 + heat
a)
Increase in the concentration of N2. Shift to the right
b)
The equilibrium mixture is heated. Shift to the left
c)
Product NH3 is removed as it is produced.
39.
Shift to the right
Write the equilibrium expression for the following reaction
CH4(s) + Cl2(g) Æ CH3Cl(g) + HCl(g)
K = [HCl]
[Cl2]
40.
Write the equilibrium expression for the following reaction.
CH4(s) + H2O(g) Æ CO(s) + 3H2(g)
K = [H2]3
[H2O]
41.
Solve the following
[NO]= 2.0M and [N2]= 2.0M
P4(s) + 6NO(g) Æ P4O6(s) + 3N2(g)
K =
[N2]3
[NO]6
(2.0)3
(2.0)6
K= 0.125 favors reactants
Show your work mole and stoichiometry questions
42.
Determine the number of grams that are in 0.688 mol of AgNO3.
Ag = 107.87 g
N = 14.01 g
O = 16.00g x 3
169.88 g/ mole
0.688 mole x
169.88g
mole
=
116.87g
How many moles of ethane (C2H6) contain 6.46 grams?
43.
C = 2 x 12.01 g
H = 6 x 1.01 g
30.08 g/ mole
6.46 g x
44.
mole
30.08 g
=
0.2147 moles
Determine the number of grams that are in 3.48 mol of NaF
Na = 22.99 g
F = 19.00 g
41.99 g/ mole
3.48 moles x
45.
41.99g
mole
=
146.125 g
For the equation below, if you have 3 moles of NH4NO3 how many moles of H2O can you
produce?
(1 step)
NH4NO3 Æ N2O + 2 H2O
3 moles NH4NO3
46.
x
=
6 moles H2O
You have 54 grams of C2H5 how many moles of H20 can you produce? (2-steps)
2 C2H5 + 5 O2 Æ
54g
x
4 CO2 + 2 H2O
1 mole C2H5
29 g
1.86 C2H5 moles x
47.
2 mol H2O
1 mole NH4NO3
=
1.86 C2H5 moles
2 moles H2O
2 moles C2H5
=
1.86 H2O moles
Use the equation given to determine how many grams of AlCl3 will be produced from 92
grams of Cl2 .(3-steps)
2 AlBr3 + 3 Cl2 Æ 3 Br2 + 2 AlCl3
92 g x
1 moles Cl2
70.9 g
1.2976 moles Cl2 x
2 moles AlCl3
3 moles Cl2
=
1.2976 moles Cl2
=
0.865 moles AlCl3
0.865 moles AlCl3 x
133.33 g
1 mole AlCl3
=
115.33 g
48.
What is the percent yield if your actual yield is 8.65 g and your theoretical yield was 9.826 g?
8.65 g
x 100 = 88.0%
9.826 g
49.
What is the percent yield if your actual yield is 5.00g and your theoretical yield was 18.75 g?
5.00 g
x 100 = 20.9%
18.75 g
50.
If 35.0g of N2O4 reacts with 19.7g of N2H4, the products will be nitrogen, N2, and water, H2O.
What mass of water, H2O, will be produced?
N2O4
+
2N2H4 Æ
3N2
+
4H2O
Solving from N2O4
35.0g
x
1 mole N2O4
92.00g
=
0.3804 moles N2O4
0.3804 moles N2O4
x
4 moles H2O
1 moles N2O4
=
1.5217 moles H2O
1.5217 moles H2O
x
18.02g
1 mole H2O
=
27.42g
Solving from N2H4
19.7g
x
1 mole N2H4
32g
0.6156 moles N2H4
x
=
0.6156 moles N2H4
4 moles H2O
2 moles N2H4
=
1.231 moles H2O
1.231 moles H2O x
18.02g
1 mole H2O
=
22.187g
N2O4 is the excess reagent
N2H4 is the limiting reagent