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CHEMISTRY FINAL 2 > FINAL > Flashcards

FINAL Flashcards

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1
Q

Diatomic element

A

The big 7

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2
Q

Simple cation

A

Single element/atom with positive charge

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3
Q

Compound

A

Group of elements

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4
Q

Poly atomic ion

A

The ions of the top of the pt

Charged group of elements

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5
Q

Multivalent ion

A

Atom with more than one charge

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6
Q

Element

A

The stuff on the periodic table

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7
Q

Families and group on pt

A

Have similar chemical properties

Are the vertical rows

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8
Q

Elements in rows/periods

A

Have respecting chemicals properties

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9
Q

What are the 5 ways to identify a chemical change

A
  1. Spontaneous change in temp
  2. Odor
  3. Formation of a gas
  4. Change in color
  5. Light
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10
Q

Precipitate

A

Solid that forms in a liquid solution

Insoluble

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11
Q

Isotopes

A

Different forms of the same element that differs by atomic mass and number of neutrons

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12
Q

What are the 7 diatomic gases

A 
H
N
O 
F
Cl
Br 
I
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13
Q

When HCL ionizes in water what ions are produced

A

H(+)

CL(+)

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14
Q

Properties of an acid

A 
Sour 
Turns litmus paper red 
Dissolves metals 
0-7 ph 
Colors in phenolphthalein
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15
Q

Properties of a base

A 
Bitter 
Slippery 
Turns litmus paper blue 
7-14 ph 
Pink in phenolphthalein 
Dissolves protiens and fats
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16
Q

Acid + metal =

A

Salt
H2
Is a single replacement reaction

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17
Q

Acid + base

A

Water
Salt
Double replacement reaction

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18
Q

Acid gives off —– ions in water

A

Hydrogen

H(+) or H3O(+)

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19
Q

Bases give off —– ions in water

A

Hydroxide

OH(-)

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20
Q

Ph of weak acid

A

6ish

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21
Q

Ph strong acid

A

1ish

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22
Q

Ph weak base

A

8ish

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23
Q

Ph strong base

A

14ish

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24
Q

Sodium hydroxide

A

NaOH

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25
Q

Sulfuric acid

A

H2SO4

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26
Q

Carbonic acid

A

H2CO3

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27
Q

Acetic acid

A

C2H4O2

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28
Q

Calcium hydroxide

A

Ca(OH)2

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29
Q

Nitric acid

A

HNO3

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30
Q

Phosphoric acid

A

H3PO4

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31
Q

Hydrologic acid

A

HCL

32
Q

Charles law

A

Gases expand when heated
When has is held at a constant pressure, the volume is proportional to the temperature
Temp increase=volume increase
Direct proportion

33
Q

Boules law

A

Volume increase = pressure decrease
Inverse relationship
The volume of a gas is in really proportional to the pressure at a constant temperature

34
Q

List four units of pressure

A

Torr
Psi
mmHg
atm

35
Q

To convert Celsius into kelvin you…..

A

K= 273 + Celsius

36
Q

Define pressure as it relates to gas

A

The force the gas exerts on the wall of it’s container

37
Q

Absolute zero

A

Lowest possible temperature
All matter/atoms stop moving
0k
273C

38
Q

What is relationship between mass and speed of gas particle

A

Mass increase = decrease in particle speed

39
Q

Gay-lussacs law

A

As temp increases= pressure increase when volume is constant

40
Q

Diffusion

A

Spread of gas thru space and substances
High concentration to low concentration
Ex) perfume smell spreading thru room

41
Q

Solution

A

Mixture of 2+ substances

Solvent + solute

42
Q

Solvent

A

Liquid where something is dissolved
Ex) the water in saltwater
Does the dissolving

43
Q

Solute

A

The substance that is dissolved in the solution
Ex) the salt in saltwater
Gets dissolved

44
Q

Dilute

A

A small amount of the solute compared to the solvent

45
Q

Concentrated

A

A large amount of solute compared to the solvent

46
Q

Kinetic energy is the energy of

A

Motion

47
Q

Potential energy is the energy of

A

Position

48
Q

Enthalpy

A

Delta H
Internal energy
The energy system produced upon reaction at constant temperature

49
Q

Entropy

A

2nd law of thermodynamics
The amount of energy that escapes durning a reaction
Disorder and chaos in system

50
Q

Activation energy

A

The energy is takes to start a chemical reaction

51
Q

Catalysts

A

Aren’t used up in reaction

Speed up a reaction by lowering the activation energy

52
Q

1st law of thermodynamics

A

Energy can’t be created or destroyed

53
Q

2nd law of thermodynamics

A

No energy system is 100% efficient
Systems seek max entropy
Entropy

54
Q

3 things to consider on the dangers of nuclear radiation

A

1) number of decays/second (half life)
2) type of radiation
3) mode of exposure~bio tissue harmed easily

55
Q

Half life

A

Time it takes for a radioactive sample to decay by half

56
Q

Alpha particle

A

Large size
Shielded by cardboard
Low penetrating power

57
Q

Beta

A

Medium size
Shielded by glass
Medium penetrating power

58
Q

Gamma

A

Small size
Shielded by many inches of lease it many feet of concrete
High penetrating power

59
Q

Short half or long half more dangerous?

A

Shorter the half life = more unstable = more radioactive = more dangerous

60
Q

Isotopes of hydrogen

A

Protium(H-1)
Deuterium(H-2)
Tritium(H-3)

61
Q

Isotopes of uranium

A

U-235 Rare

U-238 Plenty

62
Q

Where does radon gas come from

A

Decay product of U-238 and found in soil

Dangerous gas

63
Q

How many years can radiocarbon dating date an artifact

A

40,000 years

64
Q

What is used to start a fission reaction

A

Neutron

65
Q

Ionizing radiation

A

Particle flying from radioactive atom has ability to collide with molecules and knock off it’s electron

66
Q

Geiger counter

A

Used to measure radiation

67
Q

Decay/disintegration series

A

The series of radioactive decay that a substance goes through before becoming
Loses particles and energies as it become stable

68
Q

Simple anion

A

Single atom/element with a negative charge

69
Q

Equlibruim

A

Two opposing processes occur at the same rate
System will always shift to stay in equilibrium
Add a chemical=shift to opposite direction
Take away a chemical=shift towards that chemical

70
Q

Reaction rate

A

Amount/time

71
Q

Endothermic

A

Energy flows into system from surroundings
PE increase
Feels cold

72
Q

Exothermic

A

Energy flows out
Wam
PE decrease

73
Q

Enzyme

A

A catalyst in reaction rates of living organisms

74
Q

5 things that increase the reaction rate

A 
Temp increase 
Catalyst 
Increase concentration 
Increase pressure 
Increase surface area
75
Q

Combustion reaction

A

Oxygen + hydrocarbon = CO2 + water

CHEMISTRY FINAL 2 (1 decks)

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