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Chemistry > Mid Year > Flashcards

Mid Year Flashcards

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1
Q

What is chemistry?

A

The study of all substances and the changes (physical and chemical) that they undergo.

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2
Q

List the types of chemistry

A 
Organic
Inorganic
Analytical
Physical
Biochemical
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3
Q

What does organic chem deal with?

A

Substances containing carbon

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4
Q

What does inorganic chem deal with?

A

Substances without carbon

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5
Q

What does analytical chem deal with?

A

Composition of subtances

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6
Q

What does physical chem deal with?

A

Theories/experiments with chemical behavior

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7
Q

What does biochemical chem deal with?

A

Chemical processes in living things

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8
Q

Define scientific method

A

An orderly and systematic approach used to answer questions about the world around us

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9
Q

What are the steps of the scientific method?

A

1) observation –> question/purpose
2) form hypothesis
3) perform an experiment and analyze data
4) draw conclusions
5) communicate results, redo, and/or modify

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10
Q

What is the control in an experiment?

A

The group in an experiment that isn’t changed/isn’t tested for a variable and is used as a benchmark

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11
Q

What is the independent variable of an experiment?

A

Manipulated by the scientist

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12
Q

What is the dependent variable in an experiment?

A

Depends on the independent variable, the thing you measure

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13
Q

What are the parts of scientific notation?

A

A number between 1 and 10 and a power of 10

N * 10^x

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14
Q

To change from standard to scientific…

A
  1. Place the decimal point so there is one digit to the left of the decimal
  2. Number of places moved is the exponent
  3. If original number is less than 1, the exponent is negative. If it’s greater than 1, the exponent is positive
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15
Q

To change scientific to standard…

A

Move decimal point number of places in exponent. Positive= to the right. Negative= to the left.

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16
Q

All __________ digits in a measured number are significant.

A

Non-zero

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17
Q

________ in decimal numbers are never significant

A

Leading zeros

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18
Q

_____ zeros are significant

A

Sandwiched.

Between non-zero numbers

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19
Q

________ zeros in numbers without decimals are not significant

A

Trailing

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20
Q

Significant figure rule for adding and subtracting

A

The answer has the same number of decimal places as the measurement with the fewest decimal places

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21
Q

Significant figures for multiplying and dividing

A

Round (or add zeros) to the calculated answer until you have same number of sig figs as the measurement with the fewest sig figs

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22
Q

What is energy?

A

The capacity to do work or to produce heat

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23
Q

What are the types of energy (plus short description)?

A

Potential (stored)
Kinetic (in motion)
Radiant (heat, light)

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24
Q

How do we measure energy?

A

calories, BTUs, joules

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25
Q

What is a calorie?

A

Heat needed to raise one gram of water 1° centigrade

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26
Q

What is a BTU?

A

Heat needed to raise one pound of water 1° F

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27
Q

What is a joule?

A

The SI standard unit

Force of one Newton acting through one meter

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28
Q

A watt is…

A

Power of a joule of energy per second

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29
Q

1 BTU=

A

252 calories

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30
Q

1 calorie=

A

4.184 joules (J)

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31
Q

What is a Calorie?

A

1000 calories

1 kilocalorie

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32
Q

Sig figs in energy conversions

A

Sig figs in answer= sig figs in given

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33
Q

What is the law of conservation of energy?

A

Energy is neither created nor destroyed

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34
Q

What is temperature?

A

The measure of the kinetic energy of the atoms/molecules in an object

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35
Q

What are types of thermometers?

A

Bulb
Digital
Turkey popper
Galileo

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36
Q

What are the units of measurements for temperature?

A

Degrees (F and C)

Kelvins

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37
Q

°F to °C

A

°C=(°F-32) * 5/9

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38
Q

°C to °F

A

°F= (°C*9/5) +32

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39
Q

°C to K

A

°C+273= K

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40
Q

What are the states of matter?

A

Solid
Liquid
Gas
Plasma

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41
Q

Shape and volume
Kinetic Molecular Theory
Solids

A

Definite shape and volume.

Molecules are held close together and there is very little movement

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42
Q

Shape and volume
Kinetic Molecular Theory
Liquids

A

Indefinite shape, definite volume

Atoms/molecules have more space between them than a solid but less than a gas

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43
Q

Shape and volume
Kinetic Molecular Theory
Gases

A

Indefinite shape and volume

Molecules are moving in random patterns with varying amounts of distance between the particles

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44
Q

Plasma facts

A

Most common form.
Plasma In the stars and space between them makes 99% of visible universe. Used to water sterilization: no effect on taste or smell, 12 seconds

45
Q

Physical change

A

Doesn’t change chemical composition. Changes state, form, or appearance

Water freezing into ice

46
Q

Chemical changes

A

When a substance changes into something new. Signs: changes in density/melting point/freezing point, bubbling, foaming, etc.

Burning a match

47
Q

Law of conservation of matter

A

Matter is neither created nor destroyed, it only changes state or molecules are rearranged into different substances

48
Q

Intensive properties

A

Don’t depend on size of the sample of matter

Density, boiling point, color

49
Q

Extensive properties

A

Do depend on quantity of sample

Mass, volume

50
Q

What are the three classifications of substances?

A

Element
Compound
Mixture

51
Q

What is a substance?

A

Cannot be broken down or purified by physical means. Each substance has its own properties different from any other substance.

52
Q

Pure substances

A

Fixed composition and properties, can’t be separated into simpler substances by physical means. Compounds or elements.

53
Q

What are compounds?

A

Can be decomposed into smaller substances by chemical changes, always in a definite ratio

54
Q

What are elements?

A

Basic building block of matter. Cannot be decomposed into simpler substances by chemical changes

55
Q

What is a mixture?

A

Two or more substances not chemically combined. Don’t have constant melting/boiling points.

56
Q

Characteristics of mixtures

A

Variable composition
Components retain properties
May be separated by physical methods

57
Q

Homogenous mixtures

A

Look the same, but still separated by physical means

Milk

58
Q

Heterogenous mixtures

A

Relatively large pieces that are distinguishable that are easily separated by physical means
Fruit salad

59
Q

Solutions

A

Homogenous mixtures. Something is completely dissolved in something else. Best separated by distillation or evaporation. Salt water.

60
Q

Colloids

A

Like solutions. One substance trapped inside another. Identified by how they scatter light (fog). Air trapped inside the fat molecules of whipped cream

61
Q

Gravimetric filtration

A

Filtration paper in funnel in metal stand. Differences in size of components relative to size of holes. Coffee grounds

62
Q

Chromatography

A

Water creeps up strip of paper, different solubility/polarity means that some colors like to dissolve in water more and go higher up the paper. Mobile phase: water. Stationary phase: paper. Marker experiment.

63
Q

Distillation

A

Heat under round bottom flask with liquid mixture to first boiling point. Component turns to gas, rises, enters condenser. Heat transfers to tube of cold water surrounding and substance turns back to liquid and drips out. Vodka on the rocks.

64
Q

Centrifuge

A

Put vial in at angle, spin really fast, denser parts go to bottom. Blood: RBC at bottom

65
Q

Atom

A

Smallest particle of an element that retains its identity in a chemical reaction, make up all matter

66
Q

Democritus

Describe their model.

A

Greek 400 BC philosopher who said that atoms are tiny, indivisible, indestructible without experimental evidence. Just a circle

67
Q

Dalton

Describe their model.

A

English chemist and schoolteacher performed experiments to make Atomic Theory:

  1. All elements are made of indivisible atoms
  2. Same=identical. Atoms of one element are different from another
  3. Came mix physically or chemically in ratios to form compounds
  4. Chem rxs occur when atoms separate, join, rearrange. Atoms of one element never change into another
68
Q

What do you need to see it move an atom?

A

Nanotechnology called scanning tunneling electron microscopes

69
Q

JJ Thomson

A

Electrons, 1897, cathode ray tube. Cathode ray attracted to positive magnet, deflected by negative magnet, so it must be a stream of negative particles. Also discovered charge to mass ratio. Plum pudding model with the actual atom being positive

70
Q

Robert Millikan

A

Experimentally determined charge of an electron. Used Thomson’s ratio to mathematically calculate mass in 1916.

71
Q

Eugene Goldstein

A

Discovered protons. Observed a positive particle go from positive anode to negative cathode in cathode ray tube in 1896

72
Q

James Chadwick

A

Neutrons

No charge, mass equal to proton

73
Q

Ernest Rutherford

A

Nuclear model through gold foil experiment. Passed large positive alpha particles through thin sheet of gold. Most passed, a small fraction bounced back. 1911

74
Q

Atomic number

A

Number of protons

75
Q

Mass number

A

Protons plus neutrons

76
Q

Atomic mass

A

Average mass of all the isotopes

77
Q

Complete chemical symbol

A

Element symbol
Upper left mass number
Lower left atomic number
Upper right charge

78
Q

Shorthand notations of elements

A

Name-mass number
Symbol-mass number
Gold-197

79
Q

Isotope

A

Same number of protons, different number of neutrons

80
Q

3 isotopes of hydrogen

A

Hydrogen-1: 0 neutrons
Hydrogen-2: deuterium, 1 neutron
Hydrogen-3: tritium, 2 neutrons

81
Q

What device determines mass?

A

Mass spectrometer

82
Q

Amu

A

Atomic Mass Unit

1/12 the mass of a carbon-12 isotope used to define mass. A proton (and therefore a neutron) is approximately one amu

83
Q

Niels Bohr’s Model

A

Electrons are in different energy levels like rungs on a ladder and move in a fixed orbit. Further from nucleus=higher energy=closer together. Quantum=amount of energy received/released to go up/down a level

84
Q

Schrodinger

A

Made a mathematical equation to describe the behavior of electrons. Quantum mechanical model

85
Q

Quantum mechanical model

A

Determines possible allowed energies and the probability of finding electrons in different locations around the nucleus. This is the electron cloud, where the electron is 90% of the time, because the exact location at any one instant can’t be found

86
Q

S orbitals shape

A

Sphere

87
Q

P orbitals shape

A

Peanuts

88
Q

D orbitals shape

A

Double peanuts or donut around peanut

89
Q

Max number of electrons in an energy level

A

2n^2

90
Q

Electron configuration general definition

A

Arrangement of electrons in orbitals around nucleus

91
Q

Aufbau principle

A

Electrons occupy lowest levels first

92
Q

Pauli Exclusion Principle

A

Max of two electrons in each orbital spinning opposite directions

93
Q

Hund’s Rule

A

Fill each orbital in a sublevel with one electron of the same spin first, then go back and add a second of the opposite spin

94
Q

Dobereiner

A

Published a classification system of triads. The middle element had properties in between the other two
Ex: Li, Na, K reactions to water

95
Q

Mendeleev

A

Table of 60 elements arranged by properties, increasing atomic mass. Was able to predict the properties of undiscovered elements and left spaces for them

96
Q

The modern periodic table is organized by:

A

Atomic number

97
Q

Periodic law

A

When electrons are arranged in order of increasing atomic number, properties repeat periodically

98
Q

Columns, _____, or ________ share similar chemical properties

A

Groups

Families

99
Q

Three classes of elements

A

Metals nonmetals metalloids

100
Q

Metals

A 
80% of elements
Good conductors of heat and electricity
Shiny
Ductile, malleable
Solid at rt
101
Q

Nonmetals

A

Opposite properties of metals but bigger variation. Brittle, poor conductor. Most are gases at rt

102
Q

Metalloids

A

In between, conditions, like presence of another element, cause them to act one way or another

103
Q

Group 1A

A

Alkali metals

104
Q

Group 2A

A

Alkaline earth metals

105
Q

Group 7A

A

Halogens

106
Q

Group 8A

A

Noble gases

107
Q

Group 3B to 2B

A

Transition metals (d block)

108
Q

Representative elements

A

Wide range of properties. All A groups

109
Q

Inner transition metals

A

F block

Chemistry (9 decks)

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