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Chemistry 2013-2014 > Finals Flash Cards > Flashcards

Finals Flash Cards

1
Q

Matter is defined as anything that occupies space and has

A

Mass

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2
Q

Which pair Is classified as a substance

A

Elements and Compounds

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3
Q

Which of the following statements is an identifying characteristic of a mixture?

A

Can be separated by physical means

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4
Q

When sample X is passed through a filter paper, a white residue, Y, remains on the paper and a clear liquid, Z, passes through. When liquid Z is vaporized, another white residue remains. Sample X is best defined as

A

Heterogeneous Mixture

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5
Q

What best describes a chemical property of the element Iodine?

A

It reacts with Hydrogen to form a gas

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6
Q

Ductility and malleability are examples of

A

Physical Properties

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7
Q

How man kilo-joules is the equivalent of 750 joules

A

.750 kj

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8
Q

Review 8-12 in the packet

A

Skip

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9
Q

Compounds are usually broken down into their component elements by

A

Chemical Changes

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10
Q

Which Substance can be decomposed by chemical change?

A

Ammonia (Anything that is a substance and not an element)

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11
Q

What is an EXTENSIVE physical property?

A

Mass

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12
Q

How many kilo-joules of heat energy are absorbed when 100 grams of water is heated from 20 degrees Celsius to 30 degrees Celsius

A

4.18kj

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13
Q

What is the total number of joules of heat energy released when 20 grams of water is cooled from 20 degrees Celsius to 10 Degrees Celsius

A

836J

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14
Q

Homo means

A

Evenly Mixed

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15
Q

Hetero means

A

Unevenly Mixed

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16
Q

Intensive means

A

Value stays the same

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17
Q

Study 19 In Packet

A

Skip

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18
Q

An ideal gas is made up of gas particles that

A

are in random motion

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19
Q

What are the qualities of an ideal gas

A

Random Motion, Little attraction for each other, Insignificant volume, Hit wall and build up pressure, Hit each other and transfer energy but total energy remains the same

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20
Q

What are the qualities of a real gas?

A

Has volume, have force of attraction

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21
Q

Normal Units of pressure

A

STP, 1 atm, 0 degrees Celsius, 760 mmHg, 273 Kelvin, 760 torr

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22
Q

Equation for Volume Pressure, Temperature and Moles

A

V1 Phave 1 = V2 P2
____________
T1 n1 = T2 n2

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23
Q

An assumption of the kinetic theory of gas is that the particles of a gas have

A

little attraction for each other and an insignificant volume

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24
Q

The pressure on 30 milliliters of an ideal gas icreases from 101.3 kPa to 202.6 kPa at constant temperature. The new volume is equal to

A

101.3 kPa
30 mL x ________
202.6 kPa

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25
Q

A sample of gas has a volume of 2.0 liters at a pressure of 1.0 atm. When the volume increases to 4.0 liters, at a constant temperature, the pressure will be

A

.5 atm

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26
Q

a 2.5 liter sample of gas is at STP. When the temperature is raised to 273 degrees Celsius and the pressure remains constant the new volume of the gas will be

A

5.0 Liters

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27
Q

S 16 Liter sample of CH4(g) is at 0 degrees Celsius and 1 atm. The volume of the gas sample in liters at 27 Degrees Celsius and 1 atm is equal to

A

300
22.4 x _____
273

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28
Q

When 7.0 Moles of gas A and 3.0 moles of Gas B are combined, the total pressure exerted by the gas mixture is 1.0 atm. What is the partial pressure exerted by gas A in this mixture

A

.7 atm

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29
Q

Which gas will diffuse at the rate under the same conditions of temperature and pressure

A

H2

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30
Q

A .50 mole sample of CO2(g) at 2.0 atm occupies 11.2 liters. What is the temperature of the sample

A

546 K

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31
Q

The density of a gas is 3.00 grams per liter at STP What is the gram molecular mass of the gas

A

22.4g

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32
Q

What is the formula for Lead (II) Oxide

A

PbO

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33
Q

No “o”

A

Hydro

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34
Q

O

A

Hydro

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35
Q

Ate becomes your

A

Ic

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36
Q

Ite becomes your

A

Ous

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37
Q

Complete Combustion

A

—–> CO2 + H2O

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38
Q

Incomplete Combustion

A

—–> CO + H2O

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39
Q

What order you go in when balancing equation

A

HCO

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40
Q

What is the formula for Chromium (III) Oxide

A

Cr2O3

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41
Q

Which Formula is correctly paired with its Name

A

CuCl2 —–> Copper (II) Chloride

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42
Q

What is the correct name for the compound with the formula CrPO4

A

Chromium (III) Phosphate

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43
Q

What is the name of the compound whose formula is H2SO4

A

Sulfuric Acid

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44
Q

The chemical equation 4Na(s) + O2 —> 2Na^2O(s) is best described as a

A

Synthesis reaction

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45
Q

What type of reaction is illustrated by the following chemical equation 2H2O(l) —> 2H2(g) + O2(g)

A

Decomposition

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46
Q

The chemical reaction Zn(s) + CuSO4(aq) —> ZnSO4(aq) + Cu(s) is best described as a

A

Single replacement reaction

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47
Q

What type of reaction best describes the following chemical reaction 2AlCl3(aq) + 3Na2CO3(aq) —> Al2(CO3)3(s) + 6NaCl(aq)

A

Double replacement reaction

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48
Q

C2H4(g) + 3O2(g) —> 2CO2(g) + 2H2O(g)

A

Complete Combustion

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49
Q

When the equation C2H4 + 3O2 —> 2CO2 + 2H2O balanced using the smallest whole numbers, what is the coefficient of the O2

A

3

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50
Q

Al2(SO)3 + 3ZnCl2 —> 2AlCl3 + 3ZnSO4 is correctly ballanced using the smallest whole number coefficient, the sum of the coefficients is

A

9

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51
Q

KCl(aq) + AgNO3(aq) —> KNO3(aq) + X What is the correct formula for the product representing X

A

AgCl

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52
Q

In the 1880’s JJ Thomson proved the cathode ray hadn a negative charge. What subatomic particle makes up the cathode rays

A

Electrons

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53
Q

What did the discovery of cathode rays reveal about the structure of the atom

A

Made of subatomic Particles

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54
Q

Most alpha articles passed through the gold foil undeflected. What conclusion was made about the structure of the atom based on this observation

A

Mostly empty space, had to be some postive ions

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55
Q

A few alpha particles were deflected back at the source. What did this observation reveal about the structure of the atom

A

Small dense positive nucleus

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56
Q

What term refers to the region of an atom where an electron is most likely to be found

A

orbital

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57
Q

The atomic number of an atom is always equal to the total number of

A

Protons and Neutrons

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58
Q

All atoms of an element have the same

A

Atomic Number

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59
Q

The mass number of an atom is equal to the number of

A

Neutrons plus electrons

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60
Q

What is the mass number of the atom below? 3 H

1

A

3

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61
Q

Where is mass

A

On top

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62
Q

How do you find neutrons

A

Subtract two numbers

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63
Q

In which pair of atoms do both neclei contain the same number of neutrons

A

Whichever two subtract to the same number

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64
Q

What is the total number or nucleons (protons and neutrons) in the atom below

A

Top number is mass and mass is equal to protons+neutrons= Nucleons

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65
Q

What is the mass number of an atom which contains 21 electrons, 21 protons, and 24 neutrons

A

45

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66
Q

Find the average mass of a sample of magnesium which contains 78.7% Mg-24, 10.1% Mg-25 and 11.2% Mg-26

A

(24)(.787)+(25)(.101)+(26)(.112)=24.3

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67
Q

Element X has two isotopes. If 72% of the element has an isotopic mass of 84.9 atomic mass units, and 28% of the element has an isotopic mass of 87 atomic mass units, the average atomic mass of element X is numerically equal to

A

(72.0 x 84.9) (28.0 x 87.0)
___________ + ____________
100 100

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68
Q

The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (show percents) produces this average mass?

A

75%^35Cl and 25%^37Cl

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69
Q

Which electron dot symbol could represent a metalloid (B, Si, As, Te, At)

A

If it has 5 dots around it

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70
Q

The characteristics bright-line spectrum of an element is produced when its electron

A

Returns to a lower energy state

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71
Q

Which electron configuration represents a potassium ion in the excited state

A

Add up then identify element if matches, ground state if not excited

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72
Q

What is the total number of occupied sublevels in an atom of chlorine in the ground state

A

5

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73
Q

An atom has 8 electrons in a d sublevel. How many d orbitals in this sublevel are half filled

A

2

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74
Q

How do the orbitals go

A

2, 8, 18, 32, 50

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75
Q

What is the total number of sublevels in a principal energy level

A

2

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76
Q

How much does one principal energy level go up by

A

1 Each Time

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77
Q

How many protons are in the nucleus of a magnesium atom?

A

12 (atomic number)

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78
Q

Write the electron configuration for Magnesium in the ground state

A

1s22s22p63s2

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79
Q

How does an atom of magnesium become Mg+2 ion

A

Loses 2 electrons

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80
Q

What noble gas has the same electron configuration as Mg+2

A

Neon

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81
Q

Name three elements that could be X

A

Oxygen, Sulfur, Selenium

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82
Q

The pair of elements with the most similar chemical properties are

A

The ones right on top and below each other are the closest

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83
Q

Which atom has the largest atomic radius?

A

The one closest to the lower left of the table

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84
Q

As the elements of Group 16 are considered from top to bottom on the Periodic Table , the atomic radii

A

Increase and the ionization energies decrease

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85
Q

The S-2 ions differ from the S0 atom in that the S-2 ion has a

A

Larger radius and more electrons

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86
Q

What type of energy represents in the equation Na+energy—-> Na+ + e-

A

Ionization energy

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87
Q

Define Ionization Energy

A

The ionization energy is the exact quantity of energy that it takes to remove the outermost electron from the atom.

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88
Q

In which reaction is the first ionization energy greatest

A

The one closest to the top right

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89
Q

Which element in period 2 has the greatest tendency to gain electrons (electronegativity)

A

One closest to upper right

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90
Q

Period is

A

Horizontal

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91
Q

Group is

A

Vertical

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92
Q

What group in the periodic table contains the elements to the alkaline earth family

A

2

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93
Q

When oxygen combines with any alkaline metal, M, the formula of the compound produced usually is

A

MO2

94
Q

Which Element is a halogen

A

Group 7A

95
Q

Ozone is an allotropic form of the element

A

Oxygen

96
Q

Who was credited with creating the first periodic table that organized the elements according to atomic mass

A

Dmitri Mendeleev

97
Q

A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- Which particle (X or Z) most likely represents a metal atom?

A

X is metal because it becomes a smaller positive ion

98
Q

A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- which most likely represents a nonmetal atom?

A

Z because it become a larger negative ion

99
Q

Which metal is the most reactive metal?

A

The closest to the bottom left is

100
Q

Which is the most reactive non metal

A

The closest to top right

101
Q

Which element has properties of both metals and non metals

A

Any metalloid (on the line)

102
Q

Which two elements would most likely combine to form an ionic compound

A

The metal and non metal farthest from each other

103
Q

Which element can lose electrons from its two outermost energy level

A

Any transition metal (One of the metals in the middle)

104
Q

Which element exists as a monoatomic gas at STP

A

Any of the Noble Gases

105
Q

Which element exists as a diatomic gas at STP

A

C,N,O,F,Cl,Br,I,H

106
Q

Define a transition metal

A

Is more than one color and can take electrons from more than 1 energy level, can have more than one binary compound

107
Q

Given the reaction: H2 + Cl2 —-> 2HCl

Which of the following statements best describes the energy change as bonds are formed and broken in this reaction

A

The forming of the H—Cl bind releases energy

108
Q

Which formula represent an Ionic Compound

A

Any one with a metal and non metal

109
Q

If the last element is an even coefficiant what is it

A

Non polar

110
Q

If the last element is an odd coefficient what is it?

A

Polar

111
Q

Review Questions number 89-93 + Compounds in back of packet

A

SKIP

112
Q

Which combination of atoms can form a polar covalent bond?

A

H and Br

113
Q

Which two compounds contain only polar molecules

A

2 elements with odd coefficients

114
Q

In a nonpolar covalent bond, electrons are

A

Shared equally by two atoms

115
Q

Which of the following statements best explain why a CH4 molecule is non polar

A

CH4 has a symmetrical charge distribution

116
Q 
The table below shows four compounds and the boiling point of each: Which type of molecular attraction accounts for the high boiling points 
Compound | Boiling Point 
H2O             100 C
H2S             -60.7 C
H2Se           -41.5 C
H2Te           -2.2 C
A

Hydrogen Bonding

117
Q 
The table below shows four compounds and the boiling point of each: Compared the boiling points of H2S, the boiling point of H2O is relatively high. Which type of bonding causes this different?
Compound | Boiling Point 
H2O             100 C
H2S             -60.7 C
H2Se           -41.5 C
H2Te           -2.2 C
A

Hydrogen

118
Q

What is the Gram Formula Mass of Al2(SO4)3

A

342g

119
Q

What is the total number of moles contained in 115 grams of C2H5OH

A

2.50

120
Q

A sample of nitrogen containing 3.0x10^23 molecules has the same number of molecules as a sample of

A

.50 (Half) Moles of Ne

121
Q

What is the mass of 3.0x10^23 atoms of Neon

A

10 grams

122
Q

Which sample of O2 contains a total of 3.01x10^23 molecules at STP

A

16.0 grams

123
Q

The percent bny mass of oxygen in H2C2O4

A

64
____ x 100
90

124
Q

The empirical (reduced) formula of the compound whose molecular formula is P4O10

A

P2O5

125
Q

What is an empirical formula?

A

The most reduced formula

126
Q

A 10 gram sample of a hydrate was heated until all the water of hydration was driven off. The mass of anhydrous product remaining was 8.00 grams. What is the percent of water in the hydrate?

A

Second number/First Number= T
T - 100 = Answer
20%

127
Q

What is the empirical formula of a compound consisting of 29.6% Oxygen and 70.4% Fluorine by mass

A

Divide percents by the elements mass then divide the smalled number by all other numbers should equal .0 or .9 if not multiply by (5 3 5 2 5 3 5)

128
Q

A compound contains .5 moles of sodium, .5 moles of Nitrogen, and 1 mole of hydrogen. The empirical formula of the compound is

A

NaNH2

129
Q

A 16 gram sample of a compound containing only copper and sulfur is decomposed to produce 12.8 grams of copper and 3.2 grams of sulfur. What is the empirical formula of the compounds

A

Cu2S

130
Q

NaOH + HCl —> NaCl + H2O

What is the total number of grams of H2O produced when 116 grams of the product, NaCl is formed?

A

36g

131
Q

N2(g) + 3H2(g) —> 2NH3(g)

What is the total number of liters of NH3 Formed when 20 liters of N2 react completely

A

40L

132
Q

C8H16 + 12O2 —> 8CO2 + 8H2O

How many moles of H2O are produced when 11.2 liters of C8H16 gas measure at STP react completely

A

4.00

133
Q

In the reaction N2 + 3H2 —> 2NH3 how many grams of H2 are needed to produce exactly 1 moles of Ammonia

A

3 gram

134
Q

4Al(s) + 3O2(g) —> 2Al2O3(s)

Calculate the gram molecular mass of Al2O3

A

102 grams

135
Q

4Al(s) + 3O2(g) —> 2Al2O3(s)

How many moles of Al are needed for the production of 3.00 moles of Al2O3

A

6 moles

136
Q

4Al(s) + 3O2(g) —> 2Al2O3(s)

Calculate the mass in grams of 3.00 moles of Al2O3

A

306 grams

137
Q

What is the percent by mass of water present in 1.0 mole of CaSO4 o 2H2O

A

36
____ = 21%
172

138
Q

What is the total number of grams of KCl (formula mass = 74.6) in 1 liter of .200 moles solution

A

14.9 grams

139
Q

What is the molarity of a solution of KNO3 (molecular mass = 101) that contains 404 grams of KNO3 in 2.00 liters of solution

A

2.00 M

140
Q

What is the total number of solute contained in .5 liters of 3.0 M HCl

A

1.5

141
Q

How many grams of ammonium chloride (gram formula mass = 53.5 g) are contained in .500L of 2.00 liters of solution

A

53.5 grams

142
Q

How many grams of KI are dissolved in 250 grams of a 20% solution

A

50 grams

143
Q

A solution will boil at the highest temperature when it contains 1 mole of nonvolatile solute dissolved in

A

250 grams of solvent

144
Q

When 2.00 moles of sugar (C6H12O6) are dissolved in 1.00 grams of water the boiling point of the resulting solution is closest to

A

101 C

145
Q

Which solute, when qdded to 1000 grams of water, will produce a solution with the highest boiling point

A

58 grams of NaCl

146
Q

The heat of reaction (Delta H) is equal to the

A

Heat content of the products minus the heat content of the reactants

147
Q

Review 126-130 In Packet

A

SKIP

148
Q

A(g) + B(g) –> C(g)

As the concentration of A(g) increases, the frequency of collisions of A(g) with B(g)

A

Increases

149
Q

In a gaseous system, temperature remaining constant, an increase in pressure will

A

Increase reaction rate

150
Q

In an gaseous system, temperature remaining constant, a decrease in pressure will

A

Decrease reaction rate

151
Q

As the surface area of the Zn(s) used in the reaction Zn(s) + 2HCl(aq) —> ZnCl2(aq) + H2(g) is increased, the rate of the reaction will

A

Increase

152
Q

The addition of a catalyst to a reaction will cause a change in the

A

Activation Energy

153
Q

CAT (Catalyst)—>

A

ACT (Activation energy)

154
Q

Delta H

A 
- = Exo 
\+ = Endo
155
Q

Delta S

A 
- = Less Disorder 
\+ = More Disorder
156
Q

Delta G

A 
- = Spontaneous 
\+ = Non Spontaneous
157
Q

The pair of changes would indicate that a reaction is endothermic but occurs spontaneously

A

A positive Delta H and a Negative Delta G

158
Q

A chemical reaction will always occur spontaneously if the reaction has

A

Negative Delta G

159
Q

BaSO4(s) = Ba+2(aq) + SO4-2(aq)

As the concentration of the SO4-2(aq) ions increases, at a constant temperature, the concentration of Cl- Ions

A

Decrease

160
Q

CH3COOH(aq) + H2O(l) = H3O+(aq) + CH3COO-(aq)

The addition of what ion will cause the decrease in the concentration of CH3COO-(aq)

A

H3O-

161
Q

N2(g) + 3H2(g) = 2NH3(g) + heat

Which change favors the formation of ammonia?

A

Increasing the concentration of N2(g)

162
Q

2SO2(g) + O2(g) = 2SO3(g)

As the pressure is increased at the constant temperature, the number of moles of SO3(g) produced will

A

Increase

163
Q

2A(g) + B(g) + 10 kcal = C(g)

Which condition would yield the most product

A

High temperature and high pressure

164
Q

What is the equilibrium equation for the reaction 3A(g) + B(g) = 2C

A

[A]3[B]

165
Q

Which of the following is the correct equilibrium expression for
4NH3(g) + 7O2(g) = 4NO2(g) + 6H2O(g)

A

[O2]7[NH3]4

166
Q

A + B =AB

The greatest amount of AB would be produced if the equilibrium constant of the reaction is eqaul to

A

1.0x10^5

167
Q

AgI(s) = Ag+(aq) + I-(aq)

Which of the following is the correct solubility product constant expression for the reaction

A

Ksp = [Ag+][I-]

168
Q

C(s) + CO2(g) + heat —-> 2CO2(g)

Which stress on the system would favor production of CO(g)

A

An increase Pressure

169
Q

A2(g) + 3B2(g) = 2AB3(g) + heat
State two stresses that could be applied to this system that would cause this equilibrium to shift to the right. Explain why each stress would cause a shift in the equilibrium

A

Temperature and Pressure because those can change the state of the substance

170
Q

What is the pH of a solution that has an OH- ion concentration of 1x10^-9 mole per liter (Kw = 1 x 10^-14)

A

5

171
Q

What is the pH of a .00001 molar HCl solution

A

5

172
Q

If the OH- equals 1 x 10-10 at 298 k for a given soltuion, the H+ of the solution equals

A

1 x 10-4

173
Q

What s the H+ ion concentration of an aqueous solution that has a pH of 11

A

1 x 10-11 mol/L

174
Q

The H3O+ ion concentration of a solution is 1x10-5 mole per liter. This solution is

A

Acidic and has a pH of 5

175
Q

Which equation represents a neutralization reaction

A

Any equation with the product of NaCl + H2O

176
Q

What is a neutralization reaction

A

A reaction resulting in NaCl + H2O

177
Q

If 100 milliliters of .75 M HCl is required to exactly neutralize 50 milliliters of KOH, what is the concentration of the base?

A

1.5 M

178
Q

If you see exactly neutralized in an equation what do you do?

A

Multiply the first two numbers you see and then divide it by the last

179
Q

In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:
Write a balance equation for HNO3 and LiOH

A

HNO3 + LiOH —> H2O + LiNO3

180
Q

In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:If 50 milliliters of .50 M LiOH is required to exactly neutralize 100 milliliters of an HNO3 solution, what is the molarity of the HNO3 solution?

A

.25 M

181
Q

In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:What indicator was used in the titration

A

Moles

182
Q

What color does Phenothaline turn in Acid

A

Colorless

183
Q

What color does Phenothaline turn in Base

A

Pink

184
Q

What color does Litmus turn in Acid

A

Red

185
Q

What color does Litmus turn in Base

A

Blue

186
Q

Arrhenius Acid

A

Gives H+

187
Q

Arrhenius Base

A

Gives OH-

188
Q

Bronsted Lowry Acid

A

Gives H+ (Proton)

189
Q

Bronsted Lowry Base

A

Accepts H+ )Proton

190
Q

Lewis Acid

A

e- pair Acceptor

191
Q

Lewis Base

A

e- pair Donor

192
Q

How do you know what the Bronsted Lowry Bases are

A

Compare the two similar elements on each side and the one with the less H’s is the base

193
Q

In a redox reaction there is conservation of

A

Both mass and charge (everything)

194
Q

Review 161 and 162 In Packet

A

SKIP

195
Q

How do you know which substance is being oxidized?

A

Pick the first element in the equation or the metal

196
Q

How do you know a reaction is redox

A

Look for a single element and not compounds

197
Q

If there is no metal in the equation how do you know what was oxidized?

A

Look for an increase in ions

198
Q

0
e-
-1

A

Beta

199
Q

4
He
2

A

Alpha

200
Q

0
e-

1

A

Positron

201
Q

0
V
0

A

Gamma

202
Q

1

A

Beta

203
Q

2

A

Gamma

204
Q

3

A

Positron and Alpha

205
Q

To solve a Nuclear Problem what do you do?

A

Equal Everything

206
Q

What is the equation for Decay

A

TGB
——- = Decay
HL

207
Q

At the end of 12 days 1/4 of an original sample of a radioactive element remains. What is the half life of the element

A

6 Days

208
Q

An Original Sample of a radioisotope has a mass of 10 grams. After 2 days, 5 grams of the radioisotope remains unchanged. What is the half life of the radioisotope

A

2 Days

209
Q

In 6.20 Hours a 100 gram sample of Ag-112 decays to 25 grams. What is the half life of Ag-112

A

3.10 Hours

210
Q

The half life of carbon-14 is 5730 years. What fraction of a 1 gram sample of carbon-14 would remain after 17190 years?

A

1/8

211
Q 
Which quantity expresses the sum of the values below to the proper degree of precision 
 2.1
33.566
\+12.22
--------------
A

47.9g

212
Q

Using the rules for sig fig, the sum of .027g and .0023 grams should be expressed

A

.029

213
Q

What is the product of (2.324 cm x 1.11 cm) expressed to the correct sig fig

A

2.58 cm2

214
Q

During a titration, a student used 50 milliliters of .1 M acid. How many moles of acid, expressed to proper significance, were used?

A

.005

215
Q

What is the number 215 expressed in proper scientific notation with the correct number of sig fig,

A

2.150 x 102

216
Q

A student investigated the physical and chemical properties of a sample of an unknown gas ans then identified the gas. Which of the following statements represents a conclusion rather than an experimental observation

A

The gas is carbon dioxide

217
Q

What is the number 2.1 x 10^3 expressed in conventional form with the proper number of sig fig

A

2100

218
Q

The solid block shows below has a mass of 146 and a length and width of 3 and a height of 6 what is the density

A

2.7

219
Q

The process of filtration is preformed in the laboratory to

A

Separate insoluble substances in an aqueous mixture

220
Q

Linear CH4

A

CO2

221
Q

Tetrahedral

A

CH4

222
Q

Bent

A

H2O

223
Q

Trigonal Pyramidal

A

NH3

224
Q

NP

A

LDF

225
Q

P

A

DD

226
Q

Equation for moles

A

C

227
Q

Equation for Grams

A

C (mass)

228
Q

Equation for Liters

A

C (22.4)

229
Q

Equation for Molecules

A

C (6.02x10^23)

230
Q

When in Doubt

A

PV=nRT

231
Q

What is another equation for Grams

A

LP

232
Q

What is another equation for Density

A

P

Chemistry 2013-2014 (20 decks)

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