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General Chemistry 111 > Exam 1: Chapters 1, 2 and 3 Lecture Notes > Flashcards

Exam 1: Chapters 1, 2 and 3 Lecture Notes Flashcards

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1
Q

What is chemistry

A

The study of the composition and structure of materials and of the changes that matter undergoes

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2
Q

What is matter

A

Anything that occupies space and has mass

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3
Q

What characteristics of matter change during a reaction

A

Composition, structure, properties

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4
Q

What is green chemistry

A

Utilizing a set of principles that encourages alternative ways of generating new and existing chemical products without unnecessary risk to human health and population

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5
Q

What is the purpose of the scientific method

A

Experiments must be done in a controlled way so that results can be reproduced

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6
Q

What is a hypothesis

A

a statement that tries to explain something in a common way

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7
Q

What saying was Louis Pasteur known for

A

“chance favors the prepared mind”

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8
Q

What is the purpose of an experiment

A

an observation of a natural phenomena carried out in a controlled manor so that results can be duplicated and rational conclusions can be made

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9
Q

What is a theory

A

A tested explanation of a basic natural phenomenon, we cannot prove a theory to be true

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10
Q

What is a law

A

A concise statement or mathmatical equation about a fundamental relationship or occurrence in nature

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11
Q

What is the Phlogiston Theory, and an example of it

A

A theory in the 18th century that said when combustible bodies burn they release “phlogiston”

ex) wood=>burn it=>ash+phlogiston
(thought this because ash weighs less then the wood)

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12
Q

Law of Conservation of Mass

A

The total mass remains constant during a chemical reaction, and mass is neither created nor destroyed

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13
Q

Characteristics of solid matter

A
  • incompressible
  • fixed shape
  • fixed volume
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14
Q

Characteristics of liquid matter

A
  • incompressible fluid
  • no fixed shape
  • fixed volume
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15
Q

Characteristics of gas matter

A
  • compressible
  • no fixed shape
  • no fixed volume
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16
Q

What is a physical change

A
  • A change in the form of matter (not chemical identity)
  • reversible
  • no new compounds
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17
Q

What is a chemical change

A
  • transformation of one (or more kinds) of matter into a new kind of matter (or several new kinds of matter)
  • new compounds are formed
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18
Q

What is a physical property and an example of it

A

a characteristic that can be observed for a material without changing its chemical identity

ex) state of matter or color

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19
Q

What is a chemical property and an example of it

A

a characteristic of matter involving chemical change

ex) acidity or reactivity

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20
Q

Can mixtures be seperated

A

mixtures can be seperated by physical methods into 2 or more substances

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21
Q

elements

A

A type of matter that is composed of atoms with the same atomic number (# of protons in the nuclei)

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22
Q

compounds

A

a substance that contains 2 or more elements

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23
Q

What is the Law of Definite Proportions and who is responsible for it

A

In a pure compound, the elements are always present in a definite proportion or % by mass (no matter what method of preparation) (Proust)

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24
Q

Law of Constant Composition

A

a given chemical compound alwas contains its component elements in a fixed ratio

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25
Q

heterogenous mixtures and examples

A

Components vary and can seperate from eachother

ex) milk, ketchup

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26
Q

homogenous mixtures and examples

A

uniform composition and properties

ex) vodka

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27
Q

Measurment and their requirements

A

the comparison of a physical quantity, by measuring with a unit of measurement (fixed standard of measurement)

requires a measured number and the unit

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28
Q

accuracy

A

how close a measurment is to the true value

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29
Q

precision

A

how close a set of measurments are to each other

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30
Q

What digits are significant

A

all non-zero digits are significant

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31
Q

When are zeros significant

A
  • zeros betweem sig figs ex) 606
  • zeros to the right of the decimal ex) 2.0
  • 9.00 (3 sig figs)
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32
Q

When are zeros insignificant

A
  • zeros to the left of the first nonzero digit ex) .08

- zeros at the end of a nondecimal number ex)900 or 9x10^2

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33
Q

multiplication and division sig fig rule

A

smallest amount of sig figs

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34
Q

error

A

difference between the true value and what you estimated or measured

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35
Q

random error

A

scattered around average value

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36
Q

systemstic error

A

error due to equitment

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37
Q

temperature and how it flows

A

measure of “hotness”. heat flows (energy) from an area of higher temp to lower temp

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38
Q

temperature units

A
  • celsius, *C
  • fahrenheit, *F
  • kelvin, K
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39
Q

Fahrenheit to celsius conversion

A

C= 5/9 (F-32)

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40
Q

Celsius to fahrenheit

A

F=(C x 9/5) + 32

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41
Q

Celsius to kelvin

A

K=C+273.15

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42
Q

equation for force

A

massxacceleration

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43
Q

pressure

A

force per unit area

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44
Q

equation for energy

A

forcexdistance

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45
Q

equation for density

A

d=m/v

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46
Q

what is the density (and necessary temperature) of water

A

1 g/mL @ *4 C

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47
Q

What were the 4 postulates of Dalton’s Atomic Theory of Matter

A
  1. Elements consist of tiny indivisible particles called atoms
  2. An element is a type of matter of only one kind of atom, and each atom has the same properties and mass
  3. Compounds are formed when atoms of different elements combine in small whole-number rations (almost like the law of definite proportions)
  4. Chemical reactions only involve the rearrangement of atoms present in the reacting substance to give new chemical combinations (almost like the law of conservation of mass)
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48
Q

Dalton’s Law of multiple proportions

A

If 2 elements form more than one compound the ratios of the masses of the second element to a fixed mass of the first element will also be in small whole numbers

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49
Q

Discovery of the electron (3 people who proved it)

A

J.J Thompson determined the ratio of the charge to mass by generating a beam of charged particles

Robert Milikan determined the charge and mass of an electron from an oil drop experiment

50
Q

Marie Curie

A

Marie Curie coined the term “radioactivity” and discovered polonium and radium

51
Q

Plum pudding model

A
  • JJ Thompson

- said each atom consists of electrons embedded in a body of positive charge

52
Q

Ernest Rutherford’s experiment

A

used positively charged particles to bombard atoms, expecting them to pass straight through. Instead they bounced back

53
Q

what did ernest rutherford’s experiment prove

A
  • most of the mass in the gold foil was concentrated in dense areas of positively charged particles (nuclei)
  • most of an atom’s mass is the positively charged nucleus
54
Q

Physical structure of an atom

A

composed of positively charged nucleus surrounded by negatively charged electrons

55
Q

Atomic symbols

A

a 1 or 2 letter notation used to represent an element

56
Q

Isotopes

A

atoms whose nuclei have the same atomic number (protons) but a different number of neutrons (mass number)

57
Q

material

A

each of the particular kinds of matter

ex)the kind of paper or plastic

58
Q

Brief history of chemistry

A
  • making observations
  • developing materials into useful products based on observations
    ex) fire=>ceramics

-began to look at precise quantities and substances => central principle of chemistry

59
Q

atoms

A

small particles that all material is made up of

60
Q

molecules

A

precise arrangements of atoms, can build large molecules from small ones

61
Q

mass

A

quantity of matter in a material

62
Q

matter

A

whatever occupies space and can be perceived by our senses

63
Q

Antoine Lavoisier

A

the first to insist that a balance should be used in chemical research

64
Q

weight

A

the force of gravity exerted on an object. it is proportional to the mass/square of the distance between the centerof the mass of the object and the earth

65
Q

what are the 2 principle ways to classify matter

A
  • physical state (solid, liquid, gas)

- chemical composition (element, compound, mixture)

66
Q

phase

A

one of several different homogenous materials present in the portion of matter under study

67
Q

significant figures

A

the digits that include all certain digits plus a final digit having some uncertainty

68
Q

exact numbers

A

arise when you count items or when you define a unit (9 coins, not 8.5).

69
Q

atomic mass equation

A

fractional abundance x percent abundance

70
Q

mass spectrum

A

shows relative number of atoms for various masses

71
Q

percent abundance equation

A

amu= (% abundance x amu)/100

72
Q

groups (periodic table)

A

have related chemical and physical properties (columns)

73
Q

periods (periodic table)

A

possess different physical and chemical properties based on how elements react to oxygen (rows)

74
Q

endangered elements

A

other than helium, quantities of elements on earth remain constant

75
Q

what are the 8 groups of main group A elements

A
  • Alkali Metals
  • alkaline earth metals
  • boron family (triels)
  • carbon family (tetrels)
  • nitrogen group (pnictogens)
  • chalcogens
  • halogens
  • noble gasses
76
Q

what is in group b

A

transition metals

77
Q

what does the group number tell you?

A

how many electrons are in the outer shell of the element

78
Q

what are lanthanides and actinides

A

14 groups of elements that do not belong to the other 18 groups and are placed at the bottom to conserve space

79
Q

covalent bonding

A

sharing of electrons, each atom is attracted to its own nucleus and the nucleus of the 2nd atom so they share

80
Q

ionic bonding

A

result of the attraction between cations and anions

81
Q

Daltons Relative Atomic Masses, and why hydrogen

A

Dalton devised an experiment to measure an element’s mass relative to the hydrogen atom, because it was believed to be the lightest element

82
Q

Definition of AMU

A

The mass of an Atom

83
Q

Molecular formula

A

Gives the exact number of different atoms of an element in a molecule

84
Q

Structural formulas

A

show how the atoms are bonded to one another in a molecule

85
Q

Organic compound

A

Molecular substances that contain carbon combined with other elements for example hydrogen oxygen and nitrogen

86
Q

Inorganic compounds

A

compounds composed of elements other than carbon however certain carbon containing compounds are considered inorganic WTF

87
Q

how are ionic inorganic compounds named

A

The cation is always named first followed by the name of the anti on most ionic compounds contain both a metal and a nonmetal

88
Q

how are organic compounds usually named

A

according to their functional groups

89
Q

cation

A

the charge is equal to the group number

90
Q

anion

A

charge is equal to the group number -8

91
Q

do some main group metals with high atomic numbers have more than one cation?

A

yes

92
Q

do most transition metals form a cation

A

yes, more than one, one of which has a +2 charge

93
Q

when are monotomic cations given the name of the element

A

if the element forms only one cation (if more than 1 exists it can be written as a roman numeral)

94
Q

what is the stem of monotomic anions

A

-ide

95
Q

polyatomic ions

A

an ion consisting of two or more atoms chemically bonded together and carrying a net electrical charge

96
Q

formula units

A

the group of atoms or ions explicitly symbolized by its formula

97
Q

how is the formula of an ionic compound written

A

by giving the smallest possible whole-number ratio of different ions so that the combination is electrically neutral

98
Q

binary compounds

A

composed of only 2 elements

99
Q

how to write binary compounds

A

name the 1st element using the exact element name

name the 2nd element by writing the stem, with the suffix -ide

100
Q

binary acids

A

consist of a hydrogen ion and any anion

101
Q

oxide

A

an acid containing hydrogen, oxygen and another element

102
Q

hydrates

A

a compund that contains water molecules that are weakly bound in its crystals

103
Q

how are hydrates named

A
  • first named from the dry compound
  • followed by the word “hydrate”
  • followed by the prefix indicating the number of water molecules per formula unit
104
Q

chemical reactions and equations

A

a chemical equation is the symbolic representation of a chemical reaction, the number of each type of atom on the left must equal that of the right

105
Q

how to balance an equation

A
  • write the correct formula for the reactants and the products
  • balance the elements that appear once in the product
  • balance the elements that appear more than once in the product
  • check!
106
Q

molecular mass (and what kind(s) of bonds)

A

the sum of the atomic masses of all the atoms in a molecule (covalent molecules)

107
Q

formula mass (and what kind(s) of bonds)

A

the sum of the atomic masses of all atoms in a formula unit of the compound (covalent and ionic molecular compounds)

108
Q

what is the AMU of 1 carbon 12 atom

A

1 amu

109
Q

why was carbon 12 picked to be the basis of AMU

A

because it is stable, solid and nontoxic

110
Q

how to convert amu to s

A

use avogadro’s number!

6.022 x 10^23

111
Q

how much is 1 mole

A

6.022 x 10^23 things

112
Q

how many grams is 6.022 x 10^23

A

12 g

113
Q

relationship between the mass (g) to amu

A

the mass (g) of 1 mole is equal to the relative atomic mass of the element

114
Q

equation for amu and g

A

moles=mass of compound/molar mass of compound
or
moles=100g x 1 mol/x grams

115
Q

how to find the percent composition

A
  • find the milar mass

- divide mass (amu) by total mass of compound, multiply by 100

116
Q

empirical formula

A

the simplest formula for a compound. its the formula of the substances written with the smallest integer (whole number) subscripts

the percent composition of a compound leads directly to this

117
Q

limiting reagants

A

when reactants are not added according to precise stoiciometry

ultimately determines how
much product can be obtained.

118
Q

Stoichiometry

A

the calculation of the quantities of reactants and

products involved in a chemical reaction.

119
Q

Theoretical Yield

A

is the amount of product that would result if all

the limiting reagent reacted.

120
Q

Actual Yield

A

is the amount of product actually obtained from a

reaction.

121
Q

percentage yield

A

the actual yield (experimentally
determined) expressed as a percentage of the theoretical yield
(calculated).
(Actual Yield/Theoretical Yield) x 100

General Chemistry 111 (8 decks)

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