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Final Flashcards

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1
Q

What is a molecule

A

at least two atoms held together by chemical bonds (may contain atoms of the same element or different elements)

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2
Q

What is an ion

A

an atom or group of atoms with a net positive or negative charge

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3
Q

what is a cation

A

an atom with a net positive charge

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4
Q

what is an anion

A

an atom with a net negative charge

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5
Q

What is a molecular formula

A

a formula which shows the exact number of atoms of each element

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6
Q

what is an allotrope

A

one of two or more distinct forms of an element (carbon diamond and graphite)

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7
Q

what is the empiracal formula

A

a formula which tells us which elements are present in simplest whole number ratio (simplist chemical formula

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8
Q

what do organic compounds usually have

A

contain carbon in combo with elements like hydrogen, nitrogen, oxygen, and sulfur.

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9
Q

what is a cation derived from

A

metal atoms (with exception of NH4)

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10
Q

How do you name an ionic compound (compound composed of a metal cation and a nonmetal anion)

A

you say the name of the metal then add ide to the second compound

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11
Q

For ionic compounds, how do you determine the charge on the second atom

A

based on which group they’re in. (N nitride or N3- is in group 3)

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12
Q

What is a molecular compound usually composed of

A

Two nonmetal elements.

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13
Q

How do you name a molecular compound

A

Same way as a an ionic compound however you also add prefixes to the last atom (SO2 sulfur dioxide)

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14
Q

What is an acid

A

a substance which yeilds hydrogen ions (H+) when dissolved in water

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15
Q

True or false, acids always contain one or more hydrogen atom

A

true

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16
Q

hydrogen chloride (HCl) breaks up into what when dissolved in water

A

hydrochloric acid (H+ and Cl-)

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17
Q

what is avagadros number used for

A

to determine the number of atoms in something

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18
Q

what is the unit for molecular mass

A

amu

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19
Q

how do you determine amu

A

by adding up all the atomic masses

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20
Q

what is the equation for percent composition by mass of a compound

A

(the number of moles in element)(atomic mass of element)/(molar mass of compound) then mulitply the entire thing by 100%

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21
Q

How do you determine the empiracal formula of a compound when given the percent compositions

A

assume the percentage is equivalent to grams. Convert grams to moles. Then divide each solution by the smallest number of moles. Then use those answers as subscripts for each element

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22
Q

How do you go about solving a stoichiometry problem

A
  1. write the balanced equation
  2. make sure reactant are in moles
  3. use mole ratio to find number of moles formed
  4. convert moles back to grams or whaterver unit desired
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23
Q

What is a limiting reactant

A

the reactant which is used up first

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24
Q

what is the theoretical yield of a reaction

A

the amount of product which would result if the limiting reagent reacted

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25
Q

How do you calculate percent yeild

A

(actual yeild)/(theoretical yeild) x 100%

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26
Q

What is an electrolyte

A

a substance that when disolved in water can conduct electricity

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27
Q

what is a strong electrolyte

A

a compound which dissociates 100% into ions

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28
Q

Is HCL a strong weak of non-electrolyte

A

strong

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29
Q

what is ionization

A

the separation of acids and bases into ions

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30
Q

what is hydration

A

the process in whcih an ion is surrounded by water molecules

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31
Q

What is a precipitation reaction

A

A reaction which results in the formation of an insolubale product known as precipitate

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32
Q

What makes an acid

A

when a substance ionizes in water to produce H+ ions

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33
Q

What defined a base

A

the production of OH- molecules when the substance is disolved in water

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34
Q

What are a few common characteristics of acids

A
  1. sour taste
  2. cause color change
  3. react with metals
    4 conduct electricity
  4. react with carbonates and bicarbonates
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35
Q

what are some common characteristics of bases

A
  1. bitter taste
  2. slippery
  3. cause color change
    4 conduct electricity
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36
Q

According to Bronsted, what determines if something is a base or acid

A

an acid is a proton donor and a base is a proton acceptor

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37
Q

what are oxidation reduction and redox reactions considered

A

electron transfer reactions

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38
Q

What is an oxidation reaction

A

a half reaction which involves the loss of electrons

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39
Q

hat is a reduction reactions

A

a half reaction which involves the gaining of electrons

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40
Q

what is the oxidation number/state

A

the number of charges the atom would have in a molecule if electrons were transferred completely

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41
Q

What are some rules for determining oxidation numbers

A
  1. free elements (O2, K, F, H2) all have oxidation 0
  2. monoatomic ions oxidation # = charge on the ion
  3. oxygen is -2 except for (h2O2 & O22-)
  4. hyrogen is +1
  5. Flourine is -1.
  6. neutral molecule sum of oxidation #s should = 0
  7. oxidations don’t have to be integers
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42
Q

what is a combination reaction

A

when two or more substances combine to form a single product

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43
Q

what is a decomposition reaction

A

the breakdown of a compound into two or more componenets

44
Q

what is a combustian reaction

A

when a substance reacts with oxygen

45
Q

what is a displacement reaction

A

when an ion or atom is replaced be an ion or atom of a different element

46
Q

How do you determine the molarity (M) or molar concentration of a solution

A

(moles of solute )/(liters of solute) OR n/v

47
Q

How do you calculate the dilution of a solution

A

MiVi = MfVf

48
Q

True or false, ionic compounds exist as gases at 25 degrees celsius and 1 atm

A

False

49
Q

What are some properties of gases

A
  1. assume the volume/shape of container
  2. most compressible state of mater
  3. gases will mix evenly in same container
  4. gases have very low density
50
Q

what is 1 Newton equivalent to in kg

A

1 kgm/s2

51
Q

how do you calculate pressure

A

force/area

52
Q

what is boyles law

A

that the pressure of a fixed amount of gas at a constant temp is inversley proportional to the volume of the gas

53
Q

what is the relationship between pressure and volume

A

P1V1=P2V2

54
Q

what is the realtionship between volume and temperature

A

V1/T1=V2/T2

55
Q

what is r = to in the ideal gas law equation pV=nRT

A

the gas constant (0.0821 Latm/Kmol)

56
Q

how do you calculate energy

A

force*distnace

57
Q

How many Joules is 1 Kilojoule worth

A

1000J in 1 kJ

58
Q

What is relationship between pressure, temper, and volume when n is constant

A

P1V1/T1=P2V2/T2

59
Q

what is the definition of heat in chemistry terms

A

the transfer of thermal energy between two bodies that are different temperatures

60
Q

what is an exothermic process

A

any process that gives off heat

61
Q

what is an endothermic process

A

when heat is supplied to the system

62
Q

How do you determine the energy change on a system

A

energy change is (U) = heat exchange (q) and work done on or by the system (w)

63
Q

what is the equation for work in thermodynamics

A

work = -pressure (p) * change in volume (V)

64
Q

What is the conversion for Joules to Liters or atm

A

1L*atm = 101.3J

65
Q

How do you calculate change in enthalpy

A

delta H= change in U + P*change in V

66
Q

How do you calculate the enthalpy of a reaction

A

delta H = H(products)-H(reactants)

67
Q

How do you calculate heat capacity (C)

A

Heat capacity (C) = mass (m) * specific heat (S)

68
Q

what are some equations for calculating the amount of heat (q)

A

q=msAt
q=CAt

69
Q

How do you calculate the speed of a wave (u)

A

u= wavelength (lamda) * frequency (V)

70
Q

what other way can you think of an atomic orbital

A

the wave function of an electron in an atom

71
Q

What is the principal quantum number (n)

A

the energy of the orbital. Has integral orbitals like 1, 2, 3, 4, 5.

72
Q

What is the angular momentum orbital (l) and how does it relate to the principal quantum number

A

It is the shape of the orbital and it depends on what n is.

73
Q

What is the magnetic quantum number

A

describes the orientation of the oribtal in space

74
Q

what does it mean if an orbital is dimagnetic or paramagnetic

A

if it’s dimagnetic all electrons are paired and if its paramagnetic not all electrons are paired/eenrgy level is not full

75
Q

How do electron configurations correlate with group number of elemtents

A

they are the same. All elemetns in gruop 1 will have 1 valence electron and etc.

76
Q

what is the pattern of atomic radii in the periodic table

A

as you move down and to the left atomic radii increases

77
Q

Which has a larger atomic radius a cation or anion

A

anions

78
Q

what is ionization energy

A

the minimum energy required to remove an electron from a gaseous atom in its ground state

79
Q

how does ionization energy increase across the perioidc table

A

as you go up and across. same as electronegativity

80
Q

what gruop is more reactive, alkalai metals or alkalai earth metals

A

alkalai metals (1A)

81
Q

which group on the periodic table is the most stable

A

8A

82
Q

Are halogens found in elemental form in nature

A

no, they are way too reactive

83
Q

What is an ionic bond

A

the elctrostatic force that holds ions together in an ionic compound

84
Q

If an element has a low electron afinity, is it morel ikley to form cations or anions

A

cations

85
Q

if an element has a high electron afinity is it more likley to form an anion or cation

A

anion

86
Q

what group is most likley to form cations

A

alkali metals and alkaline earth metals

87
Q

what happens to the electrons in an ionic bond

A

they are trasnferred

88
Q

what is lattice energy

A

the stability of any ionic solid

89
Q

what is a covalent bond

A

A bond where two electrons are shared

90
Q

what is a lone pair

A

a pair of valence electrons that are not involved in covalent bond function

91
Q

what determines if you have a polar or non-polar covalent bond

A

The electronegativity

92
Q

what are the steps to writing a lewis structure

A
  1. write the skeletal structure with the most electronegative atom in the center
  2. count up all the valence electrons
  3. draw a single bond between the central atom and each surrounding one and complete the octets of each surrounding atom.
  4. After, if the central atom doesn’t have an octet still, add double and tripple bonds.
93
Q

What is the most likley form of a lewis structure

A

the one with the smallest/no formal charges

94
Q

what is the formal charge of an atom and how do you calculate it

A

the formal charge is the electrical difference between the valence electron an an isolated atom and the number of electrons assigned to the atom in a lewis structure.
You find it by subtracting the number of electrons drawn on the atom from the number of valence electrons the atom actually has

95
Q

give an example of a molecule which can form an incomplete octet

A

BeH2 and BF3

96
Q

give an example of a molecule which can have an expanded octet

A

SF6

97
Q

How do you determine dipole moments

A

based on eelctronegativity and the shape of the molecule

98
Q

what is hybridization

A

the mixing of atomic orbitals in an atom (usually the central one)

99
Q

How do you determine the hybridization of an orbital

A

it is equal to the number of pure atomic orbitals (Add up orbitals)

100
Q

How do you determine the hybridization of an orbital

A

it is equal to the number of pure atomic orbitals (Add up orbitals

101
Q

how many orbitals does sp3d hybrid orbitals contain

A

5

102
Q

how many pi and sigma bonds are there in a singular convalen bond

A

1 sigma bond

103
Q

how many pi and sigma orbitals are there in a double covalent bond

A

1 sigma, 1 pi

104
Q

How many pi and sigma bonds are there in a triple covalent bond

A

1 sigma, 2 pi

105
Q

what is the speed of light

A

3 x 10*8

Chem 101 (3 decks)

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