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Chemistry Flashcards

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1
Q

Chemistry

A

study of matter (what matter is made of)

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2
Q

The things that make up stuff

A

the entities that comprise matter

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3
Q

Entities (biggest to smallest)

A

atoms (protons, electrons, neutrons), molecules, electrons

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4
Q

John Dalton

A

English schoolteacher- billiard ball (sphere) model

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5
Q

The Dalton Model

A

billiard ball/sphere- atom is indivisible

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6
Q

J.J Thomson

A

raisin bun model or plum pudding

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7
Q

Plum Pudding Model

A

electrons embedded into a positive fluid

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8
Q

Cathode ray tube

A

light cannot bend by itself it needs a charge (magnetic or electric)
- showed that the mass is 2000 times smaller than a hydrogen item

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9
Q

You can calculate what with strong magnets in a circle

A

charge and mass of particles

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10
Q

Ernest Rutherford

A

the gold foil experiment

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11
Q

The Gold Foil Experiment

A

expected the beam of particles to go right through the gold foil but instead some went different ways

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12
Q

Gold Foil Experiment proved that…

A

there was a small massive centre to the atom (nucleus) that caused them to deflect

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13
Q

Nuclear Model

A

Rutherford- small positive, densely packed nucleus (over 99% of the mass in the nucleus)
Planetary

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14
Q

Niels Bohr

A

Bohr Model found by the bright line spectra

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15
Q

Bohr Model

A

nucleus and electrons orbiting (excited state)

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16
Q

Excited State

A

add electricity and the electron jumps to the higher shell from the atom absorbing energy

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17
Q

Bright Line Spectra

A

when the electrons in the excited state drop back down a certain colour is emitted based on the energy level

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18
Q

Wave Mechanical Model

A

Erwin Schrodinger

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19
Q

Number of electrons in each shell

A

2, 8, 18, 32, 32, 18, 2

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20
Q

Bohr Model outer things

A

shells or orbits or energy levels

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21
Q

Wave Mechanical Model outer things

A

orbitals (Bohr orbits)

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22
Q

Periods

A

2 elements, 8, 8, 18, 18, 32, 32

18 groups

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23
Q

Alkali metals are

A

Extremely reactive- 1

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24
Q

Alkali metals

A

Li, Na, K, Rb, Cs

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25
Q

Alkali earth metals are

A

Quite reactive- 2

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26
Q

Alkali earth metals

A

Be, Mg, Ca, Sr, Ba, Ra

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27
Q

Transition metals

A

3-12

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28
Q

Halogens are

A

extremely reactive- 17

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29
Q

Halogens

A

F, Cl, Br, I

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30
Q

Noble gases are

A

stable- 18

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31
Q

Noble gases

A

He, Ne, Ar, Kr, Xe, Rn

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32
Q

An entity is stable when…

A

the valence shell is full

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33
Q

IUPAC

A

International Union of Pure and Applied Chemistry

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34
Q

Molecular

A

two non-metals

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35
Q

Common molecular compounds

A

Sucrose- C12H22O11(s), glucose- C6H12O6(s), water- H2O(l), ammonia- NH3(g), ozone- O3(g), methanol- CH3OH(l), ethanol- C2H5OH(l)

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36
Q

Naming molecular compounds

A

use the prefixes

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37
Q

Prefixes

A
  1. Mono-
  2. Di-
  3. Tri-
  4. Tetra-
  5. Penta-
  6. Hexa-
  7. Hepta-
  8. Octa-
  9. Ennea-
  10. Deca-
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38
Q

Ionic

A

one non-metal one metal (solids)

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39
Q

Types of Ionic Compounds

A

Binary, Multivalent, Polyatomic

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40
Q

Sucrose

A

C12H22O11 (s)

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41
Q

Glucose

A

C6H12O6 (s)

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42
Q

Ammonia

A

NH3 (g)

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43
Q

Ozone

A

O3 (g)

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44
Q

Methanol

A

CH3OH (l)

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45
Q

Ethanol

A

C2H5OH (l)

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46
Q

Binary (naming)

A

two elements

- MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT

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47
Q

Multivalent (naming)

A
  • MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT AND THEN WHICH EVER OF THE TWO CHARGES YOU USED WILL BE THE ROMAN NUMERICAL
48
Q

Polyatomic (naming)

A
  • MULTIPLY THE TWO CHARGES (LITTLE NUMBERS) TO MAKE THEM CANCEL EACH OTHER OUT (using polyatomic ions)
49
Q

Acids (5 indicators that can be seen)

A
  • pH below 7 (lemon like 5 battery acid like 1)
  • turns litmus paper red
  • sour
  • react with active metals (Mg, Zn, etc.)
  • conduct electricity
50
Q

Acid Indicator (cannot be seen)

A
  • hydrogen (H)
  • COOH will always be an acid
  • all acids will be (aq)
51
Q

Base (5 indicators that can be seen)

A
  • pH above 7 (7 is neutral)
  • turns litmus paper blue
  • bitter
  • feel slippery
  • conduct electricity (electrolytes)
52
Q

Base Indicator (cannot be seen)

A
  • hydroxide (OH)
53
Q

Aqueous means…

A

dissolved in water

54
Q

Will mixing an acid and a base change the conductivity?

A
  • no

- it will produce water and electrolytes

55
Q

Every difference of one pH unit is an acidic difference of….

A
  • 10

- ex. pH 8 to 4 is 10000 times more acidic

56
Q

Isotopes

A
  • Potassium is made of 19 protons and 19 neutrons
  • some isotopes would have 21 neutrons some would have 20
  • the .1 changes the amount
57
Q

Atomic Number

A
  • tells you how many PROTONS and ELECTRONS
58
Q

Mass Number

A
  • tells you the total number of protons and NEUTRONS added
59
Q

Atomic mass minus atomic number…

A
  • tells you the number of NEUTRONS
60
Q

Why is water the universal solvent?

A
  • it is a polar substance (O is negative and H and H are positive)
61
Q

For acids ate goes to…

ide goes to….

A
  • ic

- hydro _______ ic

62
Q

If an ion is dissolved it is an ____________.

A

electrolyte

63
Q

Element

A

cannot be broken down into any other substance (one atom)

64
Q

Periods are

A

horizontal (7 of them)

65
Q

Groups are

A

vertical (18 of them)

66
Q

Do electrons farther away from the nucleus have more energy than those closer?

A

yes

67
Q

Valence electrons

A

electrons in the OUTER energy level

68
Q

Valence number

A

the number of electrons an element can gain or lose to combine with other elements

69
Q

Ion

A

an atom where the number of electrons is not equal to the protons (has a net electric charge due to the loss or gain of electrons)

70
Q

Precipitate

A

sometimes when ionic solutions are mixed they form a precipitate (a solid with low solubility that forms a solution)

71
Q

When acids and bases are mixed… (neutralization)

A

when acids and bases react together both their acidic and basic properties disappear (process of neutralization)

72
Q

Neutralization

A

acids and bases mixing and producing water and salt

73
Q

Why do ionic solids have high melting points while molecular solids have low melting points?

A
  • ionic solids have stronger attractive electrostatic (higher the attraction, higher melting point) (positive and negative attract strongly)
74
Q

Electrolyte

A

a solution that conduct electricity (ionic compounds) (ions are able to flow and move)

75
Q

Octect Rule

A

every atom wants to have 8 valance electrons in the outer most shell

76
Q

Ionic Bonding

A

when elements bond to become stable (bonds between non-metals and metals)

77
Q

Acid in Batteries

A

sulfuric acid

78
Q

Acid in Vinegar

A

acitic acid

79
Q

the most common multivalent is…

A

the top one on the chart

80
Q

Electrons are the same number as

A

protons

81
Q

Protons are the same number as

A

electrons

82
Q

bottle of hydrochloric acid means what hazard symbol

A

corrosive

83
Q

ionic are (conductor, melting point, solubility)

A

good conductor, high melting point, soluble

84
Q

neutralize stomach acid with…

A

NaHCO3

85
Q

photosynthesis formula

A

6CO2(g) + 6H2O —– 6O2(g) + C6H12O6 (exothermic)

86
Q

law of conservation of mass

A

mass of reactants and products must be the same

87
Q

reactants

A

left side of equation

88
Q

products

A

right side of equation

89
Q

endothermic

A

energy going in (takes in energy)

90
Q

exothermic

A

energy going out (lets out energy)

91
Q

cellular respiration formula

A

C6H12O6(aq) + 6O2 ——— 6CO2(g) + 6H2O(l) + energy

endothermic

92
Q

anaerobic respiration

A

(bread, pizza dough)
- yeast is the enzyme (catalyst) digesting the sugar to produce gas to make the chemical reaction occur (not part of the reaction)
C6H12O6(s) ——-
2CO2(g) + 2C2H5OH(l)

93
Q

airbags

A

energy + 2NaN3(s) ——- 2Na(s) + 3N2(g) (exothermic)

94
Q

sodium azide

A

used in airbags NaN3(s) (decomposes into its elements)

95
Q

Rusting

A

Fe(s) + O2(g) ——- Fe2O3(s)

96
Q

BBQ

A

C3H8(g) + 5O2(g) ——– 3CO2(g) + 4H2O(g)

combustion of propane

97
Q

diatomic

A

elements need (H2, Br2, etc.) in chart

98
Q

ionic compounds are (s, l, g, aq)

A

solid

99
Q

Acids are always (s, l, g, aq)

A

aqueous

100
Q

Formation

A

a + b = ab

101
Q

Decomposition

A

ab = a + b

102
Q

combustion

A

CxHy + O2(g) = CO2 + H2O

103
Q

single replacement

A

ab + c = ac + b or bc + a

104
Q

double replacement

A

(displacement or neutralization) ab + cd + cb + ad

105
Q

hydrogen w a match

A

pops

106
Q

match ____ in CO2

A

goes out

107
Q

match _____ in O2

A

gets bigger

108
Q

Moles

A

used to count atoms, particles, molecules

109
Q

Avogadro’s number (1 mol)

A

6.02 x 10 to the 23

110
Q

1 mole is defined as

A

12g of pure carbon -12

111
Q

n=m/M

A 
chemical amount (mol) = mass (g) / molar mass (g/mol) 
- mass is is amount (g), chemical amount is moles, molar mass is in periodic table
112
Q

how to find atoms or molecules

A

multiply the moles by 6.02 x 10 to the 23

113
Q

How to read 2Na(s) + 2H2O(l) ——- H2(g) + 2NaOH(aq)

A

“2 moles of sodium react with 2 moles of water to produce 1 mole of hydrogen and 2 moles of sodium hydroxide”

114
Q

How to find # of particles

A

n x N (moles times Avogadro’s number)

115
Q

when writing equations do you put the positive or negative element first?

A

Positive

116
Q

round to…

A

the same number of digits as the question gives you

Science 10 (7 decks)

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