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Chemisrty 1006 > Chapter 1-4, 6 > Flashcards

Chapter 1-4, 6 Flashcards

1
Q

Physical Change

A

A change that alters only the state or appearance of a substance, but not its chemical composition
Ex: change in state from liquid to gas

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2
Q

Chemical Change

A

A change that alters the molecular composition of a substance

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3
Q

Physical Property

A

A property that a substance displays without changing its chemical composition
Ex: melting point

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4
Q

Chemical Property

A

A property that a substance displays only by changing its composition via a chemical change
Ex: combustibility

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5
Q

Kinetic Energy

A

Energy associated with motion

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6
Q

Potential Energy

A

Energy associated with its position or composition

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7
Q

Thermal Energy

A

Energy associated with the temperature of an object

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8
Q

Law of Conservation of Energy

A

Energy can neither be created nor destroyed, only converted from one form to another

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9
Q

Units

A

The standard quantities used to specify measurements

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10
Q

International System of Units (SI)

A

The standard unit system used by scientists, based on the metric system

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11
Q

How do you measure something?

A

Measure to the number of markings on the measurement device then estimate to the next digit

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12
Q

Significant Figures

A

In any reported measurement, the place holding digits that indicate the precision of the measured quantity
* the greater the number of sig figs, the greater the certainty of the measurements

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13
Q

Name the sig fig rules

A
  • all non zero digits are significant: 28.03 has 4 SF
  • zeros between non zero digits are significant: 408.1 has 4 SF
  • zeros to the left of the first non zero digit are not significant (they only serve to locate the decimal point): 0.0032 has 2 SF
  • Zeros after a decimal point are always significant: 45.000 has 5 SF
  • zeros before a decimal point and after a non zero digit are always significant: 140.00 has 5 SF
  • Zeros before an implied decimal point are ambiguous and scientific notation should be used
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14
Q

Exact numbers

A

Numbers that have no uncertainty and thus do not limit the number of SF in any calculation
Ex: 3 atoms means 3.0000000… atoms

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15
Q

SF in multiplication and division calculations

A

the result carries the same number of SF as the factor with the fewest SF

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16
Q

SF in subtraction and addition calculations

A

the result carries the same number of decimal places as the quantity with the fewest SF

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17
Q

SF in logarithmic and natural calculations

A

the result has the same number of SF after the decimal point as there are SF in the number whose log is being calculated. The digits before the decimal place in the answer represent the order of magnitude
Ex: log(4.5250 x 10^1)= 1.65562

the same is true for natural calculations

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18
Q

SF in antilogarithm calculations

A

the number of SF in the result is the same as the number of SF after the decimal place. The number before the decimal place represents the order of magnitude.
Ex: 10^6.125=1.33x10^6

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19
Q

Precision

A

refers to how close a series of measurements are to on another or how reproducible they are

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20
Q

Accuracy

A

refers to how close the measure value is to the actual value

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21
Q

Law of Conservation of Mass

A

matter can neither be created no destroyed, only rearranged

- atoms combine in simple whole number ratios to form compounds

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22
Q

Atomic Theory (John Dalton)

A
  1. Each element is composed of tiny indestructible particles called atoms
  2. all atoms of a given element have the same mass and physical/ chemical properties that distinguish them from the atoms of other elements
  3. atoms combine in simple whole number ratios to form compounds
  4. atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms only change the way they are bound together with other atoms
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23
Q

Electron

A

a negatively charged, low mass particle found outside the nucleus

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24
Q

Nucleus

A

the very small, dense core of the atom that contains most of the atom’s mass and all of its positive charge, contains protons and neutrons

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25
Q

Proton

A

positively charged subatomic particle found in the nucleus

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26
Q

Neutron

A

a electrically charged neutral subatomic particle found in the nucleus, with a mass almost equal to that of a proton

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27
Q

Atomic Number (Z)

A

the number of protons in a nucleus

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28
Q

Chemical Symbol

A

a unique one or two letter abbreviation for each element

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29
Q

Isotope

A

atoms of the same element with the same number of protons, but different number of neutrons and different masses

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30
Q

Natural Abundance

A

the relative percentage of a particular isotope in a naturally occurring sample with respect to other isotopes of the same element

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31
Q

Mass Number (A)

A

the sum of the number of neutrons and protons in an atom

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32
Q

Atomic Mass

A

the average mass in u of the atoms of a particular element based on the relative abundance of the various isotopes; it is numerically equivalent to the mass in grams of one mole of the element

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33
Q

Nuclear theory

A

the theory that most of the atom’s mass and all of its positive charge is contained in a small dense nucleus

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34
Q

Unified atomic mass unit (u)

A

a unit used to express the masses of atoms and subatomic particles

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35
Q

ion

A

an atom or molecule with a net charge cause by the loss of gain of electrons

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36
Q

cation

A

a positively charged ion

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37
Q

anion

A

a negatively charged ion

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38
Q

mole

A

a unit defined as the amount of material containing 6.022 x 10^23 (avogadro’s number) particles

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39
Q

Molar mass

A

the mass (g) of one mol of atoms of an element usually equivalent to the atomic mass of the element in u

molar mass= 1 mol
molar mass/ 1 mol

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40
Q

Converting between mols and atoms

A

1 mol/ 6.022 x 10^23
or
6.022 x 10^23/1 mol

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41
Q

main group metal

A

tends to lose electrons and forms cations with the same number of electrons as the nearest noble gas

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42
Q

Main group non metal

A

tends to gain electrons and form anions with the same number of electrons as the nearest noble gas

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43
Q

ionic bond

A
  • occur between metals and non metals

- involves the transfer of electrons from one atom to another

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44
Q

covalent bond

A
  • occur between 2 or more non metals

- involves the sharing of electrons between 2 atoms

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45
Q

Chemical formula

A

a symbolic representation of a compound which indicate the elements present in the compound and the relative number of atoms of each

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46
Q

empirical formula

A

a chemical formula that shows the simplest whole number ratio of atoms in the compound

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47
Q

molecular formula

A

a chemical formula that shows the actual number of atoms of each element in a molecule of a compound

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48
Q

structural formula

A

a molecular formula that shows how the atoms in a molecule are connected or bonded to each other

49
Q

Polyatomic ion

A

an ions composed of two or more atoms

50
Q

Ion compound

A
  • ionic compounds always contain positive and negative ions
  • in a chemical formula, the sum of the charges of the cations must equal the sum of the charges of the anions
  • a formula reflects the smallest whole number ratio
51
Q

How do your write the formula for ionic compounds

A
  • write the symbol for the metal cation and its charge followed by the symbol for the non metal anion and its charge
  • adjust the subscript on each cation and anion to balance
  • check the sum of the charges

Al^3+. O^2-
Al2O3
Cations- 2(3+)= 6+
Anions- 3 (2-)=6-

52
Q

How do you name ionic compounds?

A

-identify the compound as an ionic compound (metal +non metal)
- name the metal first, if the metal can form cations with different charges, add the charge in roman numerals
- name the non metal and add the suffix “ide”
CrBr3
Chromium (III)
Chromium (III) bromide

53
Q

How do you name polyatomic ionic compounds?

A
  • identify the compound as a polyatomic ionic compound (metal +polyatomic0
  • use the same rules as naming normal ionic metals
  • use the name of the polyatomic ion
    NaNO2
    Sodium
    Sodium nitrate
  • if the compound contains both a polyatomic cation and anion use the names of both
    NH4NO3
    ammonium nitrate
54
Q

Acid

A

a molecular compound that donates H+ ions when dissolved. Composed of hydrogen and one or more non metals

55
Q

binary acids

A

composed of hydrogen and a non metal

56
Q

how do you name binary acids

A

hydro + base name of the non metal + “ic acid”

hydrobromic acid

57
Q

oxyacid

A

composed of hydrogen and an oxyanion (non metal + oxygen)

58
Q

how do you name an oxyacid

A

oxyanion ending in “ate’- base name of axyanion + “ic acid”
- nitric acid

oxyanion ending in “ite’ - base name of oxyanion + “ous acid”
- sulfurous acid

59
Q

Formula Mass

A

the average mass of a molecule

60
Q

Mass Percent Composition

A

an element’s percentage of of the total mass of a compound containing an element

mass percent of element x = (mass of element x in 1 mol of compound/ mass of 1 mol of compound)(100)

61
Q

Empirical Formula Molar Mass

A

the sum of the masses of all atoms in an empirical formula

62
Q

Combustion Analysis

A

a method of obtaining empirical formulas for unknown compounds, especially those containing carbon and hydrogen, by burning a sample of the compound in pure oxygen and analyzing products of the combustion reaction

63
Q

Chemical reaction

A

a process in which one or more substances are converted into on or more different ones

64
Q

Combustion reaction

A

a type of chemical reactions in which a substance combines with oxygen to form one or more oxygen containing compounds

65
Q

chemical equation

A

a one line expression that shows the reactants and products in a chemical reaction

66
Q

reactant

A

substances that are consumed in a chemical reaction

67
Q

products

A

the substances produced in a chemical reaction; they appear on the right hand side of the chemical equation

68
Q

solvent

A

the majority component of a solution

69
Q

solution

A

a homogenous mixture of 2 substances

70
Q

solute

A

the minority component of a solution

71
Q

aqueous solution

A

a solution in which water acts as the solvent

72
Q

molecular equation

A

an equation showing the complete neutral formula for each compound in a solution

73
Q

complete ionic equation

A

an equation which lists individually all of the ions present as either reactants or products in a chemical equation

74
Q

spectator ions

A

ions in a complete ionic equation that do not participate in the reaction and therefore remain in the solution

75
Q

net ionic equation

A

an equation that shows only the species that actually change during the reaction

76
Q

acid base reaction

A

a reaction in which an acid reacts with a base and the 2 neutralize each other, producing water

77
Q

neutralization

A

the state of a solution where the concentrations of H3)+ and OH- are equal

78
Q

Arrhenius definitions of acids and bases

A

the definitions of an acid as a substance that produces H+ ions in aqueous solution and a base as a substance that produces OH_ ions in an aqueous solution

79
Q

hyrdronium ion

A

H3O+ the ion formed from the association of a water molecule with an H+ ion donated by an acid

80
Q

polypro tic acid

A

an acid that contains more than on ionized proton and releases them sequentially

81
Q

oxidation reduction reaction

A

reactions in which electrons are transferred from one reactant to another and the oxidation states of certain atoms are changed

82
Q

oxidation

A

the loss of one or more electrons; also the gaining of oxygen or the loss of hydrogen

an increase in oxidation state

83
Q

reduction

A

the gaining of one or more electrons; also the gaining of hydrogen or the loss of oxygen

a decrease in oxidation state

84
Q

oxidation state

A

a positive or negative whole number that represents the charge an atom in a compound would have if all shared electrons were assigned to the atom with a greater attraction for those electrons

85
Q

oxidation agent

A

oxidizes another substance (is reduced)

86
Q

reducing agent

A

reduces another substance (is oxidized)

87
Q

limiting reactant

A

the reactant with the smallest stoichiometric amount in a reactant mixture and consequently limits the amount of product in a chemical reaction

88
Q

theoretical yield

A

the greatest amount of product that can be made in a chemical reaction based on the limiting reactant

89
Q

percent yield

A

the percentage of the theoretical yield of a chemical reaction that is actually produced

90
Q

actual yield

A

the amount of product actually produced by a chemical reaction

91
Q

molarity (M)

A

a means of expressing solution concentration as the number of moles of solute per litre of solution

92
Q

Stock solution

A

a highly concentrated form of a solution used in laboratories to make less concentrated solutions via dilution

93
Q

concentrated solution

A

a solution that contains a large amount of solute relative to the amount of solute

94
Q

dilute solution

A

a solution that contains a very small amount of solute relative to the amount of solvent

95
Q

thermochemistry

A

the study of the relationship between chemistry and energy

96
Q

energy

A

the capacity to do work

97
Q

heat (q)

A

the flow of energy caused by a temperature difference

98
Q

thermal energy

A

a type of kinetic energy associated with the temperature of an object, arising from the motion of individual atoms or molecules

99
Q

kinetic energy

A

energy associate with motion of an object

100
Q

potential energy

A

energy associate with the position or composition of an object

101
Q

chemical energy

A

energy associated with the relative positions of electrons and nuclei in atoms and molecules

102
Q

law of conservation of energy

A

energy can neither be created or destroyed, bu it can be transferred from one object to another

103
Q

system

A

a specific area of interest

104
Q

surroundings

A

everything else

105
Q

the first law of thermodynamics

A

the total energy in the universe is constant

106
Q

internal energy (u)

A

the sum of kinetic energy and potential energies of all of the particles that compose a system

107
Q

state function

A

a function whose value depends only on the state of the system, not on how the system got to that state

108
Q

Heat capacity (c)

A

the quantity of heat required to change a system’s temp by 1 degree

109
Q

specific heat capacity

A

the amount of heat required to raise the temp of 1 gram of a substance by 1 degree

110
Q

pressure volume work

A

work that occurs when a volume change takes place against an external pressure

111
Q

bomb calorimeter

A

a piece of equipment designed to measure delta u for combustion reactions at constant volume

112
Q

enthalpy (H)

A

the sum of the internal energy of a system and the product of its pressure and volume; the energy associated with the breaking and forming of bonds in a chemical reaction

113
Q

exothermic reaction

A

a chemical reaction that releases heat to its surrounds

delta h is less than 0

114
Q

endothermic reaction

A

a chemical reaction that absorbs heat from its surroundings

delta h is greater than 0

115
Q

coffee cup calorimeter

A

a piece of equipment designed to measure delta h for reactions at a constant pressure

116
Q

hess’s law

A

the law stating that if a chemical equation can be expressed as the sum of a series of steps, then delta h for the overall equation is the sum of the enthalpies of reactions for each step

117
Q

standard state

A

for a gas the standard state is the pure gas at a pressure of exactly 1 bar; for a liquid or solid the standard state is the pure substance in its most stable form at a pressure of 1 bar and the temperature of interest; for a substance in solution the standard state is a concentration of exactly 1 mol/L

118
Q

standard enthalpy change

A

the change in enthalpy for a process when all reactants and products are in their standard states

119
Q

standard enthalpy of formation

A

the change in enthalpy when 1 mol of a compound forms from its constituent elements in their standard states

Chemisrty 1006 (1 decks)

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