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Lydia's Brainscape Decks > CHEM EXAM!! > Flashcards

CHEM EXAM!! Flashcards

1
Q

What is density?

A

The amount of space (volume) and object takes up in relations to how many particles (mass) is in the object.

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2
Q

Precision

A

Degree to which repeated measurements under unchanged conditions show the same results.

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3
Q

Accuracy

A

Degree of closeness of a quantity to the actual (true) value.

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4
Q

What is mass?

A

A quantity which measures how much matter or particles are inside a certain object. Measure of the “insides” of something

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5
Q

What is volume?

A

The amount of space that an object takes up. Its what contains the elemnts and parts of that object.

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6
Q

Metric conversions prefixes

A

M-mega 10^6, k-kilo 10^3, h-hecto 10^2, da-deca 10^1, B-base, d-deci 10^-1, c-centi 10^-2, m-milli 10^-3, u-micro 10^-6, n-nano 10^-9

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7
Q

Whats an volumetric flask?

A

Flask with round sides

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8
Q

What is molar mass?

A

The mass of 1 mole of any chemical compound or element. 6.02x10^23 molecules, atoms, etc. Each atom times the mass on there periodic table, then add all together.

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9
Q

Erlenmeyer flask

A

Flask with straight sides

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10
Q

What is PASS?

A

P-pull pin
A-aim at base of fire
S-squezze
S-sweep back and forth

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11
Q

What can you observe in a physical change?

A

1: State 2: Shape 3:Size

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12
Q

Chemical property

A

Can be observed by changing the identity of the substance.

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13
Q

Physical change

A

Changes form of the substance without changing the identity. Chemical properties stay the same.

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14
Q

What can you observe in a chemical change?

A

light, heat, cooling, color, odor, bubbles, solid, smoke

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15
Q

What is an Alloy?

A

homogeneous mixture of metals

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16
Q

Element

A

composed of a single atom ( smallest particle of an element will obtain all of its properties)

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17
Q

Compounds:

A

Composed of two or more elements combined together in a specific ratio

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18
Q

Physical property

A

Can be observed without changing the identity of a substance.

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19
Q

Chemical change

A

Changes the identity of a substance. Products have different properties.

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20
Q

Homogeneous mixture:

A

uniform in composition every portion is like every portion (solution)

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21
Q

`Observation

A

Anything you know based on your five senses.

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22
Q

Inference

A

An educated guess based on your five senses.

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23
Q

Heterogeneous mixture:

A

composition varies from position to position

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24
Q

Cation

A

positive charge

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25
Q

Exothermic

A

Gives off heat energy. Ex: hand warmers

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26
Q

Endothermic

A

Uses heat energy Ex: ice pack

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27
Q

Solute

A

A substance dissolved in a solution. Ex: Salt

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28
Q

Solvent

A

Substance that dissolves a solute. Ex: water

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29
Q

Solution

A

Homogenous mixture that may contain solid, liquid, gas.

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30
Q

Filtrate

A

Material, usually liquid, that has passed through a filter.

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31
Q

Precipitate

A

Formation of a solid in a solution.

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32
Q

Law of conservation of mass

A

Mass is neither created nor destroyed, only changed.

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33
Q

Anion

A

negative charge

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34
Q

What is an isotope

A

elements that have a difference in their neutrons and therefor mass/stability

35
Q

For anion naming in isotopes

A

Drop ending of the element and ad ide and then ion

36
Q

Filtration

A

Filtrate passes through filter, residue is left behind.

37
Q

Evaporation

A

Heat the solution until solvent evaporates leaving behind the solid residue.

38
Q

For cation naming

A

Add ion to the element name

39
Q

For transition metal naming

A

there are multiple charges so we use roman numerals name (numeral) ion

40
Q

Atomic mass

A

Weighted average of all the isotopes for an element. amu

41
Q

Relative abundance

A

The frequency of the isotopes occurring in nature.

42
Q

Ous ending

A

a lower charge

43
Q

Ic-ending

A

higher charge

44
Q

What is a nuclear reaction

A

Changes the composition of the atoms nucleus due to the nucleus being unstable

45
Q

Radiation

A

Emission of energy as electromagnetic waves or subatomic particles.

46
Q

Radiocativity

A

-spontaneous emission of radiation from a atom

47
Q

Nuclear stability

A

-associated with p+ and n*
-strong nuclear forces
-p+ repelling p+ electro magnetic repulsion
-n have no electrical repulsion so they act as a glue holding the nucleus together
- elements 1-20 p=n stable
-past 20 more n required
-past 80 radioactive due to p and n balance.

48
Q

Properties of Alpha radation

A

-2 p 2 n
-mass of 4 amu
-charge +2
-when you gain/lose the element changes
-slower due to a larger mass
-when their is to many p and high repulsion

49
Q

Beta radiation:

A

-high speed e- from nucleus
-n split into p and e
-mass o
-charge -1
-occurs when an n needs to be kicked out

50
Q

Democritus

A

Gave the term “atom”. Current def: An atom is the smallest particle of an element that retains the chemical identity of the element.

51
Q

Dalton

A

Used Lavoisier’s law of conservation of matter and Proust’s law of constant comp. the create his 4 point theory. 1. All matter consists of tiny particles called atoms. 2. When elements react, the combine in simple whole number ratios. 3. Atoms are indestructible and unchangeable. 4. Elements are identified by their atoms. All atoms of a given element are identical. 3 and 4 are now proven incorrect.

52
Q

Franklin

A

Stationary electric charge, two kinds of electrical charge (+ and -).

53
Q

Thomson

A

Experimented with currents of electricity inside empty glass tubes (cathode ray tubes). Discovered sum atomic particles. The cathode rays were made up of electrons.

54
Q

Gamma Radation

A

-high energy
-not made of particles
-mass 0 charge 0
-electromagnetic radiation
-typically goes with alpha/beta

55
Q

Fission

A

splitting
-large nucleus breaks into 2 or more small pieces
A+B –> C
-emission/decay

56
Q

Fusion

A

combine
-small moving particles fuses with the nucleus
A+B=C
-capture/bombard

57
Q

Half life

A

average amount of time for half a sample to decay

58
Q

Bequerel/Curies

A

Discovered radiation from uranium, radium, and polonium. Showed that atoms could be changed. Alpha, beta, gamma.

59
Q

Milikan

A

Oil drop experiment. Measured the charge and mass of an electron. Found mass and charge of the electron.

60
Q

Rutherford

A

Gold foil experiment. Discovered that the atom has a dense, positive center and most of the atom is empty space. Discovery of proton.

61
Q

Chadwick

A

Discovered the neutron.

62
Q

Bohr

A

Flame tests and spectrum. Electrons travel in definite energy levels (orbitals) instead of random motion.

63
Q

Schrodinger

A

Concept of electron clouds.

64
Q

Atomic emission spectrum

A

-spectrum with only certain colors
-finger print of an element

65
Q

Continuous Spectrum

A

contains all colors on in order of freq. /wavelength

66
Q

Max Planck

A

studied light emitted from heated objects
connected energy and frequency

67
Q

Quanta

A

atoms can gain or lose energy in specific amounts

68
Q

E(quanta)=hv

A

E- quanta
h-planks constant 6.626 * 10 -34
v-frequency (hz)

69
Q

Quantum theory

A

light energy comes in specific amounts (packets)
photons- packets of em radiation
photoelectric effect-electrons are ejected from surfaces of metals when certain frequencies of light shine on metals

70
Q

Light production

A

1: e at ground state lowest energy level and most stable
2: add energy
3: e jump to a higher energy energy state excited state
4: e drop back down and resale the added energy as light

71
Q

The energy levels

A

there are 7
each energy level has sub levels
s(low e-),p,d,f(high e-)
2 electrons max per orbital

72
Q

Electromagnetic radiation

A

Forms of energy that exhibit wave like behavior as it travels

73
Q

Order of electro. radiation in order of increasing frequency

A

radio, radar, micro,infrared, visible, ultraviolet, x-ray, gamma

74
Q

Wavelength

A

Shortest distance between equivalent points on a continuous wave. Crest to crest etc.

75
Q

Quantum numbers

A

n=principle energy level
L= energy sub level/shape (s,p,d,f)
ml= orientation in space p^x, p^x
ms= electron spin

76
Q

Bohr’s energy equation

A

E=Rh(1/ni-1/nf)
e-energy of jump/fall (J)
Rh-rydbergs constant 2.18 *10^18
ni=intail enery level
nf=final energy level

77
Q

Frequency

A

Number of waves that pass a given point per second. Hertz. 1Hz=1wave/1sec

78
Q

Amplitude

A

Height from rest position to crest/ trough.

79
Q

Speed

A

s=wavelength x frequency (c= 3.00x10^8 m/s)

80
Q

Liters in mole conversions

A

22.4 L

81
Q

Particles in mole conversions

A

6.02 x 10^23 particles

82
Q

Paula Exclusion Principle

A
  • an orbital can only hold 2 electrons and they must have opposite spin
83
Q

Aufbau Principle

A

electron fill lowest energy orbitals first

84
Q

Hunds Rule

A

electrons fill equal energy orbitals one at a time only pairing when they have too ( e- repel e-)

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