Download Review - Discount Flies

Review
Chapter 2:
Scientific and Standard Notation
Units and conversions - convert 200 cm to meters
Sig Figs: how many sig figs in:
0.0031050 pounds
25010 meters
Multiply/Divide:
3x4 = ?
3.0 x 4.0 = ?
Add/Subtract:
+
3.1
45
48.1
+/- .1
+/- 1
= ?
Chapter 3:
States of matter: solid, liquid, gas
Physical Property - property of matter that can be determined without
changing the compound. i.e. Color, smell, density, …
Chemical Property – property of matter that is determined by changing the
substance. i.e. Flammability, corrosiveness,..
Physical Change – Change in state of matter i.e. melt water
Chemical Change – Change a substance to a different substance
i.e. burn something
Element – 1 type of atom
Compound – 2 or more different elements that make up a molecule
Homogenous Solution – solution that is the same throughout. i.e. Salt and
water
Heterogenous Solution – solution that is different throughout. i.e. Dirt and
water.
Examples of Energy: heat, light, motion, nuclear,..
measured in units of: joules, calories,
Calories
Specific Heat – The amount of energy needed to raise 1 gram of a substance 1 oC.
Problem: Determine the Calories needed to warm 27 g of iron by 4 oC.
q = ms∆t
q = (27 g) ( .45 J
g oC
= 48.6 J x
)
(4 oC)
1 calorie x
1 Calorie =
4.184 J
1000 calories
0.0116 Calories
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Chapter 4:
Proton, Neutron, Electron characteristics: Relative mass, and charge
Isotopes:
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How many protons, neutrons and electrons are in:
Names of group 1, 2, 17, 18,
3
Li +
3-12 ,
1-2 and 13-18 and charges of each group.
Metals, metalloids and non-metals
cation vs anion
Chapter 5: Nomenclature
Polyatomic ions:
Type 1 metal & non-metal naming rules
ClO3- Cr2O7-2 OH-
NO3- NH4+
Type 2 metal & non-metal rules
Name the following:
Non-metal & non-metal rules
FeSO4
Name the following:
Ca(OH)2
MgCl2
KH2PO4
Cu 2O
P2O5
Write formulas for the following:
Write formulas for the following:
Manganese (II) nitrate
Sodium oxide
Zinc phosphate
Iron (III) sulfide
Ammonium phosphate
Nitrogen dioxide
Naming acids:
Without oxygen:
hydro ______________ ic acid
HCl?
HBr?
With oxygen:
ic acid
if anion ends with ate
H NO3?
Root + ous acid
Root +
if anion ends with ite
H NO2?
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Chapter 6: Chemical Reactions:
Write a balanced equation for the following reaction:
Methane gas reacts with oxygen gas to produce carbon dioxide and water.
Chapter 7: Aqueous solution reactions:
Know the solubility chart and how to determine if something is soluble in
water.
Write a molecular, complete and net ionic equation for:
A solution of barium chloride and sodium phosphate are added.
Chapter 8: Types of Reactions:
Redox – transfer of electrons from 1 substance to another
Mg + Cl2 MgCl2
CH4 + O2 CO2 + H2O
Double Replacement:
AB + XY AY + XB
Acid-Base:
HA + BOH
Acid-Carbonate:
HA + BCO3 BA + HOH + CO2
BA + HOH
Zn + HCl ZnCl2 + H2
Single Replacement:
ZnCl2 + H 2 ???
Combustion:
HC
+ O 2 CO2 + H2O
Metal + O2 Metal Oxide
A + B AB
AB
A + B
Synthesis:
Decomposition
Chapter 9: Moles
Convert 10.0 g Al to moles
10.0 g Al x 1 mole = .37 mole Al
27.0 g
Convert 10.0 g Al to atoms
10.0 g Al x 1 mole Al
27.0 g
x 6.02 x 1023 atoms Al = 2.23 x 1023 atoms Al
1 mole Al
Define atomic mass
Define molar mass
What is the molar mass of water?
3
Convert 22 g H2O to moles H2O
22 g H2O x
1 mole H2O
18 g H2O
=
1.2 mole H2O
Convert 22 g H2O to molecules of H2O
22 g H2O x
1 mole H2O x 6.02 x 1023 molecules H2O = 7.2 x 1023 molecules
18 g H2O
1 mole H2O
How many atoms of H are in 22 grams of H2O?
22 g H2O x
1 mole H2O x 6.02 x 1023 molecules H2O x 2 atoms H
18 g H2O
1 mole H2O
1 molecule H2O
= 1.4 x 1024 atoms of H
A compound has a molar mass of 216 g/mole and for every 6.22 g of Nitrogen, it
has 17.8 g of Oxygen. Determine its empirical and molecular formula.
Empirical formula:
6.22 g N x 1 mole = .444 mole N / .444 mole = 1 mole x 2 = 2 mole N
14 g
17.8 g O x 1 mole = 1.11 mole O / .44 mole
16 g
= 2.5 mole x 2 = 5 mole O
Therefore, the empirical formula is N2O5, which has a molar mass
of 28 + 80 = 108 g/mole
216 = 2
108
2 (N2O5) = N4O 10
(check to see that N4O10 weighs 216 g/mole)
Determine the percent composition of N in ammonium nitrate.
NH4NO3 has
%N =
gN
g everything
2 mole N
4 mole H
3 mole O
=
= 28.0 g
= 4.0 g
= 48.0 g
80.0 g
28.0 x 100 = 35 % Nitrogen
80.0
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Chapter 10: Stoichiometry:
12.15 g of Mg is added to 16 g O 2. Predict the g of MgO formed
12.15 g Mg x
Avail:
1 mole = .50 mole Mg
24.3 g Mg
.50
16 g O2 x
1 mole = .50 mole O2
32 g O2
.50
2 Mg + O2 2MgO
Case 1
Case 2
.50
1.0
.25
.50
.50
1.0
which doesn’t work?
.50 mole MgO x 40.3 g MgO = 20. g MgO forms
1 mole MgO
% Yield: Regarding the problem above, the reaction is completed, and 17 g MgO
is formed from the experiment. What is the theoretical, actual and
percent yield?
= 17 x
% Yield = actual
theoretical
20
Theoretical = 20. g
100 = 85 %
Actual = 17 g
Chapter 11: Atomic Theory
Properties of waves: (wavelength, amplitude, frequency, speed)
Different types of light are determined by their wavelength…radio, uv, infrared,
visible, x-ray,..
Electron principle energy levels n = 1 , 2 , 3 , …
Sub energy levels: s
p
d
f
Electron configuration and orbital diagram for:
S
How many unpaired electrons?
S-2
Size: Increases going down a group, decreases going left to right
Ionization Energy – the energy required to remove an electron from an atom.
decreases going down a group, increases going left to right across a period.
Electronegativity – increases
toward fluorine
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Chapter 12: Bonding
Intramolecular – bond between atoms to form a molecule
Covalent
Polar Covalent
Ionic
bond between HCl?
electronegativity difference
0 - .2
.2 - 1.7
> 1.7
H2O?
NaF?
Intermolecular – bond between 2 molecules
Lewis structures of molecules:
What is the shape of: H2S? CO2? PH 3?
molecular shapes:
Linear
Trigonal Planar
Tetrahedral
Trigonal Pyramidal
Bent
Chapter 13: Gases
Know the relationship between pressure and volume plus temperature and
volume.
Combined Gas Law: deals with changing conditions.
P1V 1 = P2V2
T1
T2
Calculate the volume of 2 liters of gas at 100 oC and 3 atm if it is changed to STP.
(3 Atm) (2 L)
(373 K)
=
(1 Atm) (V2)
(273 K)
V2 = 4.4 Liters
2 Liters of gas at 3 atm is converted to 1 atm of pressure. What is the volume?
(3 Atm) (2 L)
= (1Atm) (V2)
Temperature is not changed, and is eliminated
in the equation.
V2 = 6 Liters
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Pressure units and conversions
Convert 275 mm Hg to atm
275 mm Hg
x
1 torr
1 mm Hg
x
1 atm = .362 atm
760 torr
Ideal Gas Law: P V = n R T used mostly when moles, grams, molecules or
atoms are included in the problem.
Determine the volume of 2.0 g of He at STP
2.0 g He x 1 mole = .5 mole He
4.0 g
(1 atm) (V) = (.50 mole) (.0821) (273)
11.2 liters
R = .0821 (atm)
8.31 (kPa)
62.36 (torr)
Partial Pressure:
2 mole of H2 and 3 mole of N2 are placed into a container with a total pressure
of 1.0 Atm. What is the partial pressure of the H2?
Pi = Xi Pt
PH2 = 2 (1 atm) = .4 atm
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Gas Stoichiometry:
3 Liters of CH4 are mixed with 2 Liters of O2 at STP. How many moles of CO2
will form at STP?
Avail: 3 L
CH4
Case 1 3
Case 2 1
+
2 L
2O2 CO2 +
6 won’t work
2
1
1 Liter of CO2:
2H2O
PV = nRT
(1 atm) (1 Liter) = n (.0821) (273)
n = .0446 mole CO2 forms
Kinetic Molecular Theory:
1.
2.
3.
4.
Gas particles are small relative to the space they travel in.
Molecules move in straight line motion, changed by collisions.
Collisions are elastic.
Velocity of molecules is dependant on temperature.
Diffusion: movement of gas molecules from high to low concentration.
Lighter molecules have higher average velocity than heavy molecules,
therefore, light molecules diffuse faster. (Taco Bell)
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Chapter 14: Solids and Liquids
∆Hfusion = 6.02 kJ/mole
∆Hvaporization = 40.6 kJ/mole
How much energy is required to warm 18 g ice at 0oC to 100oC steam?
18 g x 1 mole x 6.02 kJ x 1000 J = 6,020 J
18 g
1 mole
1 kJ
q = 18 g x 4.184 J x 100 oC
g oC
= 7,531 J
18 g x 1 mole x 40.6 kJ x 1000 J = 40,600 J
18 g
1 mole
1 kJ
6,020 + 7,531 + 40,600 = 54,151 J
Polarity of a molecule is determined by its shape and the electronegativity of
the elements that make it up.
Intermolecular Bonds:
1.
2.
3.
4.
Dipole-Dipole
Hydrogen
London
Ionic
What type of bonding would be
found in molecules of:
HCl?
H2S?
H2?
H2O?
Vapor Pressure – function of molecular weight and strength of intermolecular
bonding.
Which has higher vapor pressure, CH3OCH3 or CH3CH2OH? (Can you name
these compounds?)
Solids are classified by their bonding:
Ionic –
metal + non-metal
Molecular –
non-metals
Atomic –
network or metallic (diamond or iron)
What type of solid is: NH3? BaO?
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Chapter 15: Solutions
Dissociation
Concentration is usually measured by Molarity, M
M = mole solute
Liters solution
Calculate the molarity of 11.5 g NaOH dissolved in 1.5 Liters solution
11.5 g NaOH x 1 mole = .2875 mole NaOH
40.0 g
M = .2875 mole = .19 M NaOH
1.50 L
Solution Stoichiometry
What mass of KNO3 is formed from .0035 mole Ba(NO3)2 added to
265 mL .010 M K2CrO4?
.010 M = mole
.265 L
M = mole
Liter
mole = .00265
Avail: .0035 mole
Ba(NO3)2
Case 1 .0035
Case 2 .00265
.00265 mole
+ K2CrO4 .0035
.00265
BaCrO4
+
.00265
2KNO3
(2)(.00265) = .0053
.0053 mole KNO3 x 101.1 g = .53 g KNO3 will form
1 mole
Chapter 16: Kinetics, Equilibrium and Solubility
A + B C
350
200
100
What is Ea and ∆H for the forward reaction? Is this endothermic or exothermic?
What about the reverse reaction? ( C A + B)
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Equilibrium – Forward and reverse reaction occur at the same rate
Write the Equilibrium expression for 2H2O(l) ↔ 2H2(g) + O2(g)
K = [H2]2 [O2]
Small K means that reaction favors reactants, large K favors product formation.
LeChateliers Principle
A(s) + 3B(g) ↔ 2C(g) + D(aq) + energy
add B
remove A
increase P
lower temperature
The solubility of PbF 2 is 2.5 x 10-3 mole/Liter. Calculate Ksp
PbF2(s) ↔ Pb+2
2.5 x 10-3
2F-
+
(2) 2.5 x 10-3 = 5 x 10-3
Ksp = [Pb+2]
[F-]2
[2.5 x 10-3][5 x 10-3]2
= 6.3 x 10-8
Chapter 17 – Acids and Bases
Acid – H+ donor
Base - H+ acceptor
Write an equation of water + ammonia.
Strong acids dissociate completely, weak acids barely dissociate.
Write an equation of
HCl
HF
+ H2O
+
H2O
Know the list of strong acids.
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Auto-ionization of water:
H2O + H2O
H 3O+ + OH-
Kw = 1 x 10-14 = [H+][OH-]
What is the [H+] and pH of a .25 M NaOH solution?
NaOH Na+ + OHInit
Final
.25
0
0
.25
0
.25
1 x 10-14 = [H+][.25]
[H+] = 4 x 10-14
pH = (-1) log 4 x 10-14
= 13.4
Does this make sense?
Mg + Cl2 MgCl2
What is oxidized?
What is reduced?
What is the oxidizing agent?
What is the reducing agent?
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