Chem 101 - Test 1

Front 1

1 kg = ? lbs

Back 1

2.2 lbs

Front 2

1 in = ? cm

Back 2

2.54 cm

Front 3

K = C + ?

Back 3

K = C + 273.15

Front 4

F = C?

Back 4

F = 1.8C + 32

Front 5

V of cylinder = ?

Back 5

V = pi(r^2)h

Front 6

standard deviation = ?

Back 6

= SQRT((SUMd^2)/(n-1))

Front 7

10^6=(name and symbol)

10^3=

10^2=

10^1=

Back 7

Mega (M)

kilo (k)

hecto (h)

deka (da)

Front 8

10^-1=

10^-2=

10^-3=

10^-6=

10^-9=

10^-12=

Back 8

deci (d)

centi (c)

milli (m)

micro (u)

nano (n)

pico (p)

Front 9

1 L = ?qt

Back 9

1.057 qts

Front 10

1 mL=?cm^3

Back 10

1 cm^3

Front 11

1 gallon = ?qts

Back 11

= 4 qts

Front 12

can K be (-)?

K is proportional to...

Back 12

NO

the average amount of kinetic energy

Front 13

in the solid state,

Back 13

atoms and molecules pack closely in a fixed location

Front 14

a homogenous mixture has...

Back 14

uniform composition and properties throughout

Front 15

a heterogenous mixture has...

Back 15

different substances that remain physically seperate

Front 16

a chemical change is...

Back 16

when a substance combines with another substance, either through synthesis or decomposition

Front 17

a physical change only...

Back 17

affects the form of a substance, not it's chemical composition. It often involves state changes (liquid, gas, or solid)

Front 18

a physical property is...

Back 18

any measurable property whose value describes the state of a physical system (density)

Front 19

kinetic energy is best defined as...

Back 19

the energy of motion

Front 20

intensive and extensive properties???

Back 20

need more info

Front 21

exact numbers...

Back 21

can be considered to have an infinite number of significant figures

Front 22

ionic:

covalent:

Back 22

metal + nonmetal (cation + anion)

nonmetal+nonmental (use prefixes)

Front 23

Free element charge:

2 exceptions to charges:

Back 23

0

hydrogen in hydrides, where H = -1 (when H is bonded to a metal, it acts as a nonmetal)

peroxides (e.g. H2O2), where O acts as -1

Front 24

3 transition metals that have definite oxidation states (don't need parentheses):

Mercury is written as:

Back 24

Cd2+, Zn2+, Ag+

Hg2^2+

Front 25

acetate

ammonium

Back 25

C2H3O2(-)

NH4(+)

Front 26

carbonate

chromate

Back 26

CO3(2-)

CrO4(2-)

Front 27

hypochlorite

chlorite

chlorate

perchlorate

Back 27

ClO(-)

ClO2(-)

ClO3(-)

ClO4(-)

Front 28

cyanide

dichromate

Back 28

CN-

Cr2O7(2-)

Front 29

dihydrogen phosphate

hydrogen carbonate

Back 29

H2PO4(-)

HCO3(-)

Front 30

hydrogen phosphate

hydrogen sulfate

Back 30

HPO4(2-)

HSO4(-)

Front 31

hydroxide

oxalate

Back 31

OH-

C2O4(2-)

Front 32

Nitrite

Nitrate

Back 32

NO2(-)

NO3(-)

Front 33

permanganate

peroxide

Back 33

MnO4(-)

O2(2-)

Front 34

phosphate

sulfite

sulfate

Back 34

PO4(3-)

SO3(2-)

SO4(2-)

Front 35

Sb

As

Ba

Be

B

Br

Back 35

Antimony

Arsenic

Barium

Beryllium

Boron

Bromine

Front 36

Ga

Au

Kr

Ne

Ni

Pd

Back 36

Gallium

Gold

Krypton

Neon

Nickel

Palladium

Front 37

Pt

Pu

Ra

Rn

Rb

Back 37

Platinum

Plutonium

Radium

Radon

Rubidium

Front 38

Sr

W

U

Zr

Back 38

Strontium

Tungsten

Uranium

Zirconium

Front 39

Properties of solids: 4:

Back 39

fixed shape, fixed volume, can't be compressed or flow

Front 40

Properties of liquids: 4:

Back 40

indefinite shape, fixed volume, can't be compressed, can flow

Front 41

Properties of gas: 4:

Back 41

indefinite shape, indefinite volume, can be compressed, can flow

Front 42

Close packing of matter leads to________, while loose packing leads to _________.

Back 42

definite volume and shape, indefinite volume and shape

Front 43

2 kinds of solids and what makes them different:

Examples: 2 of each

Back 43

crystalline - molecules are arranged in an orderly, geometric patter. Amorphous - pattern of molecules is not arranged at all.

crystalline examples: salt and diamonds

amorphous examples: plastic, glass, charcoal

Front 44

Liquids are ________ packed, making them ________.

Back 44

tightly packed, making them incompressable. This allows liquids to take the shape of the container, but does not allow them to escape and expand to fill container like a gas.

Front 45

In a gas state, particles are free from each other, there is a lot of __________ between particles. Because of this, particles can be _________ and gas can __________ to fill a container.

Back 45

empty space, compressed expand

Front 46

a pure substance is ________ whose __________ does not change from one sample to another. It is made of a single type of ______ or _______. All samples have the same ________.

Back 46

matter whose composition does not change. atom or molecule. All samples have the same characteristics.

Front 47

________ whose composition varies from one _____ to another is called a ____________. It has ________ combined in __________. Because the composition varies, ____________.

Back 47

Matter, sample, mixture. 2 or more types of atoms or molecules combined in VARIABLE PROPORTIONS. samples have different characteristics.

Front 48

substances that cannot be broken down into simpler substances by chemical reactions are called__________

substances that can be decomposed are called_________. Most pure substances are _______________.

Back 48

elements - composed of single kind of atom although may be O2, etc.

compounds. They are combinations of elements and molecules. All molecules of a compound are IDENTICAL so all samples of a compound behave in the same way.

Compounds.

Front 49

Difference between a mixture and a compound?

Back 49

A mixtures physical properties are not consistent because it has different molecules in varying degrees.

A compound's properties are always the same because it consists of 2 or more atoms, but IDENTICAL molecules. Most pure substances are made of this.

Front 50

A pure substance can be an _______ or a ____________, as long as it has only one kind of substance.

Back 50

element, compound

Front 51

A _________ mixture describes one that has uniform composition throughout. Every piece of the sample has ________.

A_________ mixture does not have uniform composition. It contains regions with _________ and the atoms and molecules_______

Back 51

homogenous, the same characteristics

herterogenous mixture, different characteristics, atoms and molecules are not mixed uniformly.

Front 52

A good way to tell a homogenous mixture is one that is made of multiple substances but appears to be one substance.

Back 52

see other side

Front 53

Pure substance vs.____________

Element vs. __________

homogenous mixture vs. _____________

Back 53

mixture

compound

heterogenous mixture

Front 54

Match the physical change to it's lab technique:

boiling point -

state of matter -

adhereance to surface

volatility

density

Back 54

distallation

filtration

chromatogrpahy

evaporation

centrifugation and decanting

Front 55

changes that alter the state or appearance of the matter without altering the composition are called_________

changes that alter the composition of the matter are called_________

Back 55

physical changes

chemical changes - atoms rearrange into new molecules, but all original atoms are still present

Front 56

the characteristics of matter that can be changed without changing its composition____________.

the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy are ___________

Back 56

physical properties (density, mass)

chemical properties (polarity)

Front 57

__________ force is the push or pull on objects that have an electrical charge.

Back 57

electrostatic force

Front 58

_______ energy is due to the composition of matter and its position in the universe.

Back 58

potential - it arises from electrostatic forces between atoms, molecules and subatomic particles

Front 59

materials that posses _______ potential energy are less ________.

processes in nature tend to occur on their own when the result is material(s) with lower total potential energy

Back 59

high, less stable

Front 60

1. Zero’s between numbers are significant. 30.09 has 4 SF

2. Zero’s that precede are NOT significant. 0.000034 has 2 SF

3. Zero’s at the end of decimals are significant. 0.00900 has 3 SF

4. Zero’s at the end without decimals are either. 4050 has either 4 SF or 3 SF

Back 60

see other side

Front 61

________ is an indication of how close a measurement comes to the actual value of the quantity. It produces ___________.

__________is an indication of how reproducible a measurement is. It produces ______.

Back 61

accuracy, systematic

precision, random errors

Front 62

______ believed matter was infinitely divisible while ________ believed that matter had a tiny, indivisible particle.

Back 62

Aristotle, Democritus

Front 63

Law of conservation of mass:

Back 63

matter can neither be created nor destroyed - it all must add up in the end

Front 64

Law of definite proportions

Back 64

a chemical compound always contains the exact same composition by mass

Front 65

Law of Multiple Proportions

Back 65

when two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers. For example, there are five distinct oxides of nitrogen, and the weights of oxygen in combination with 14 grams of nitrogen are, in increasing order, 8, 16, 24, 32, and 40 grams, or in a ratio of 1, 2, 3, 4, 5.

Front 66

Dalton's Atomic Theory:

Each element is composed of_______

All atoms of a given element have the same __________ and ______ that are unique to that element

atoms combine in________

In a chemical reaction, atoms of one element cannot__________

Back 66

tiny, indestructible particles called atoms

mass and properties

simple, whole number ratios to form molecules and compounds

change into atoms of another element

Front 67

the number of protons in the nucleus of an atom is called the _______

the percentage of an element that is 1 isotope is called the isotope’s _________

Back 67

atomic number

natural abundance. Note: the only thing different is the mass. All isotopes are CHEMICALLY identical

Front 68

________ behave much differently than the neutral atom

When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically

This is associated with __________

Back 68

ions

periodic law

Mendeleev

Front 69

Metals are _______ at room temp (except Hg), conduct _______ and ________. Are ______, ______, and ________. The ______ e- to form cations.

Back 69

solids

heat and electricity

shiny, malleable, ductile

lose electrons

Front 70

Nonmetals are found in ______. They are poor conductors of _____ and _______. Solids are _________. They ___ e- to become anions.

Back 70

all 3 states, heat and electricity

brittle

gain

Front 71

_____ show some properties of metals and some of nonmetals. They are also known as ______

Back 71

metalloids

semiconductors

Front 72

Despite its position on the periodic table, ____ is a nonmetal

Back 72

hydrogen

Front 73

Columns of the periodic table are called ___ or ______ while rows are called ______.

Back 73

groups or families

periods

each period shows the pattern of properties repeated in the next period

Front 74

Transition Elements vs. _______ or ______

B vs. ____

Back 74

Main Group or Representative Elements

A

Front 75

Back 75

Purples = alkalai metals

Blue = alkali earth metals

Yellow = transition metals

Green = nonmetals

Brown = metalloids

Orange = non metal

beige = halogens

light blue = inert elements/ noble gases

off-white = lanthanides then actinides

Front 76

hydrogen forms _____ with nonmetals and ______ with metals

Back 76

compounds, hydrides (where it's charge is -1)

Front 77

Alkali metals are ____ and have ____ boiling points and _______.

The are very ________ and almost never found uncombined in nature.

They react with water to form ____ aka _______ solutions.

Back 77

soft, low boiling points and density.

reactive.

basic aka alkaline

Front 78

Alkali earth metals are ______, _____ melting and ______ than alkali metals.

They are _______, but less so than alkali.

form stable, insoluble oxides from which they are normally extracted

Back 78

harder, higher melting and denser.

reactive.

Front 79

All halogens are _________ and _______

Back 79

nonmetals, diatomic

Front 80

Noble gases are all gases at _______. The have low ___ and _____ points. They are very _____.

Back 80

room temperature. low melting and boiling points. unreactive.

Front 81

The atomic mass is the sum of the _________ times _______.

Back 81

fractional abundance of the isotope times the mass of the isotope

Front 82

masses and abundances of isotopes are measured with a ________

a _______ is a graph that gives the relative mass and relative abundance of each particle

Back 82

mass spectrometer

mass spectrum

Front 83

Avogadro’s Number = 6.0221421 x 1023

First list all atoms in order of metals, nonmetals, then “H” & “O” last. Leave the species that is split between more than one compound for last.

Back 83

see other side

Front 84

Change Observation

formation of a precipitate solid is formed

formation of water heat is formed

formation of a gas bubbles formed

other changes are:

Electrochemistry electrons are transferred

Thermochemistry heat is transferred

Back 84

see other side

Front 85

IONIC EQUATIONS have the substances which exist as ions written in ionic form. H+ (aq) + Cl- (aq) + Na+ (aq) + OH-(aq) → Na+ (aq) + Cl- (aq) + H2O (l) Precipitation, Acid/base, and Redox reactions can all be written depicting the appropriate substances as ions

NET IONIC EQUATIONS are ionic equations with the Spectator ions removed. H+ (aq) + OH-(aq) → H2O (l)

SPECTATOR IONS do not participate in a reaction (that is they do not react to form a new substance). Common Spectator ions are Group I, many Group II, and NO3- (nitrate) and C2H3O2- (acetate) ions.

Back 85

see other side

Front 86

% X = (total atomic mass of X / molar mass which contains X)

Back 86

see other side

Front 87

soluable vs _________

miscible vs ________, which means that the substances easily mix to form a uniform solution or that they separate into 2 distinct layers.

a solution is a _________ mixture.

Back 87

insoluble

miscible vs immiscible

homogenous

Front 88

The solute remains uniformly distributed throughout the solution and will not settle out through time.

if the attractions between solute and solvent are strong enough, the solute will dissolve

Back 88

see other side

Front 89

________ dissociate into ions when dissolved. ___________ do not dissociate when dissolved.

Back 89

ionic compounds. molecular compounds.

Front 90

______ are species which conducts electricity when dissolved in water

strong acid, bases and salts are ________

weak acid and bases are ________

Back 90

electrolytes

strong electrolytes

weak electrolytes

Front 91

ENDPOINT = POINT OF NEUTRALIZATION = EQUIVALENCE POINT

At the end point for the titration of a strong acid with a strong base, the moles of acid (H+) equals the moles of base (OH-) to produce the neutral species water (H2O). If the mole ratio in the balanced chemical equation is NOT 1:1 then you must rely on the mole relationship and handle the problem like any other stoichiometry problem.

Back 91

see other side

Front 92

titration technique:

known solution in buret:

Back 92

volumetric analysis

titrant

Front 93

The concentration of the titrant must be known (called the standard solution).The exact reaction between the titrant and reacted substance must be known.The equivalence point must be known. An indicator that changes color at, or very near, the equivalence point is often used.The point at which the indicator changes color is called the end point. The goal is to choose an indicator whose end point coincides with the equivalence point. NOTE: Equivalence Point ≠ End Point! WHY???5. The volume of titrant required to reach the equivalence point must be known (measured) as accurately as possible.

Back 93

see other side

Front 94

P = F/A

1 atm = 760 mmHg = 760 torr = 14.69 psi = 101.3 kPa

Boyle’s Law P1V1 = P2V2

Charles’ Law V1 / T1 = V2 / T2

Guy-Lussac’s Law P1 / T1 = P2 / T2

Avogadro’s Law V1 / n1 = V2 / n2

Combined Gas Law P1V1 / T1 = P2 V2 / T2

Back 94

Pressure = force per area unit

Front 95

Dalton's Law of Partial Pressures: Ptotal = Pgas A + P gas B + Pgas C …

PA = χAPTotal.

dSTP = molar mass/molar volume

d = (MM) P / R T

Back 95

see other side

Front 96

root mean square speed = SQRT (3RT/MM) where R = 8.3145 J/K mol

KE per mole = 3/2 RT

Back 96

see other side

Front 97

Heavy molecules (such as CO2) travel with speeds close to their average values. The greater the molar mass, the lower the average speed and the narrower the spread of speeds. Light molecules (such as H2) not only have higher average speeds, but also a wider range of speeds.

Back 97

Maxwell distribution of speeds

Front 98

Rate of effusion of gas A = √(molar mass B / molar mass A) Rate of effusion of gas B

Back 98

see other side

Front 99

a ________ is the quantity of heat required to change the temperature of one gram of water by one degree Celsius

Back 99

calorie

Front 100

1 cal = 4.184 J

1000 cal = 1kcal

The third law of thermodynamics:The entropy of a perfect ________ at 0 K is _______.There is __________ at absolute 0 K.

Back 100

crystal, 0. no molecular movement

Front 101

____________ gives off heat

____________ takes in heat

Back 101

exothermic

endothermic

Front 102

___________ is the same of all the kinetic/ potential energy in a system

_______ is the variable for heat added to or liberated from the system. A positive variable, means that heat is being ______ while a negative means heat is being _______ to surroundings. This holds true for w too.

Back 102

internal

q, added. transferred

Front 103

─Work = External Pressure x Change in Volume

State Function: In this case, it does not matter how crazy it was getting from A to B. It only matters what initial and final values were. It is important to know when it is a state function and when it is not. E.g. boiling water - doesn’t matter how water got from cold to hot, just the difference. State function means life it easier! Enthalpy is a state function

Back 103

see other side

Front 104

Hess’s LawIf a reaction is carried out in a series of steps, ΔH for the reaction will be equal to the sum of the enthalpy changes for the individual steps.

Back 104

see other side

Front 105

decomposition is endothermic because heat is needed to break bonds. synthesis is exothermic.

Back 105

see other side

Front 106

formation of the elements trick still applies - if elements are present, be wary that the value is probably zero.

Back 106

see other side