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berlin b > unit 3 test science > Flashcards

unit 3 test science Flashcards

1
Q

what is energy?

A

capacity to do work

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2
Q

potential energy

A

energy stored in an object due to position
ex: chemical potential energy

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2
Q

kinetic energy

A

energy that has motion
ex: light, sound, mechanical

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3
Q

law of conservation of energy
AKA: first law of thermodynamics

A

energy cannot be created or destroyed only transformed from one form to another

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4
Q

second law of thermodynamics

A

when energy is transformed some heat energy is lost

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5
Q

matter

A

anything that has mass and occupies space

can be a solid,liquid,or gas

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6
Q

what is matter made of?

A

atoms

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7
Q

what is an atom?

A

basic / smallest unit of matter

cannot be counted - too many

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8
Q

democritus and John dalton

A

came up with the stages of atomic theory

democritus started ideas

John dalton named them

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9
Q

atomic theory: 1

A

all matter is made of indestructible particles called atoms

atomos means invisible

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10
Q

what model is shown in atomic theory 1?

A

Solid sphere model

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11
Q

what is energy

A

capacity to do work

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12
Q

kinetic energy

A

energy that has motion

ex: light, sound, electrical, mechanical

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13
Q

potential energy

A

energy stored in an object due to position

ex: chemical potential energy

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14
Q

first law of thermodynamics
(law of conservation of energy)

A

energy cannot be created or destroyed only transformed from one form to another

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15
Q

second law of thermodynamics

A

when energy is transformed some energy is lost as heat

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16
Q

what is matter made of?

A

atoms

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17
Q

what is an atom?

A

basic / smallest unit of matter

cannot be counted since there are so many

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18
Q

democritus and John dalton

A

created the atomic theory

democritus came up with the ideas

dalton tested / named his ideas

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19
Q

which model was created by John dalton / democritus?

A

solid sphere model

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20
Q

atomic theory 2

A

all atoms of the same element are identical in size, shape, and mass.

weight determines size

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20
Q

atomic theory 1

A

all matter is made of indestructible particles called atoms

atomos means invisible

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21
Q

atomic theory 3

A

atoms cannot be created or destroyed in chemical reactions - they just rearrange

ex: wood burns -> ash / gas

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22
Q

atomic theory 4

A

in a chemical reaction atoms of one element combine with atoms of another to form compounds

they can only be formed in wholes no halves

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23
Q

what experiment did JJ Thomson do and what did he find out?

A

cathode ray experiement

electrons are negatively charged

cathode ray has negative charges; it attracts positive / repels negative

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24
Q

plum pudding model

AKA Chocolate chip cookie model

A

created by JJ Thomson

positive background with negative charges throughout

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25
Q

what experiment did Ernest rutherford do and what did he find out

A

gold foil experiment

atom is mostly empty space and the mass is at the center (nucleus)

nucleus has positive charges (protons)

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26
Q

nuclear model

A

created by ernest rutherford

positive center with negative throughout

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27
Q

what did Neil Bohr believe?

A

electrons travel in orbits of fixed size and energy

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28
Q

what experiment did Neils Bohr do and what did he find out?

A

emision spectrum

electrons go around nucleus in orbits

electrons will admit lower energy closer to nucleus and higher when farther

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29
Q

planetary model

A

created by Neils bohr

positive center/nucleus

rings of electrons with various energy levels

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30
Q

quantum model

A

created by Erwin shrodinger

we cannot find exact location of electrons

electrons are located in 3D clouds

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31
Q

what experiment did James Chadwick do and what did he discover?

A

shooting protons at beryllium

discovered the nuetron

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32
Q

what model is used today?

A

Bohr’s model / planetary model

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33
Q

electron orbitals

A

electrons surrounding nucleus

where chemical bonding and reactions occur

33
Q

nucleus

A

center of atom

where nuclear reactions occur

34
Q

proton

A

positively charged particle in the nucleus

mass of 1.0073 amu/atomic mass unit (approx 1 g/mol)

same as atomic number

symbo;l is p+

35
Q

neutron

A

neutral particle found in the nucleus

mass of 1.0087 amu/atomic mass unit (approx 1 g/mol)

number of neutrons determines isotopes

symbol is n^0

36
Q

electron

A

negatively charged particle that occupies a 3D region around the nucleus (orbitals)

mass of 5.5 x 10^-4 amu/atomic mass unit (approx 0 g/mol)

electrons are involved in chemical reactions

symbol is e-

37
Q

what is volume created by in the atom?

A

electron orbitals

38
Q

valence electrons

A

electrons in the outermost shell/ring - involved in forming bonds

39
Q

isotopes

A

atoms of the same element with a different number of neutrons (giving a dif mass)

has the same number of protons but different number of neutrons

40
Q

atomic mass or mass number

A

total mass of an atom

atomic mass = p + n

measured in amu (atomic mass unit)

41
Q

standard nuclear notation

A

z^aX

X - chemical symbol for number

A- mass number / rounded avg. mass number

Z- atomic number / number of protons (number below name)

42
Q

nuclear chemistry

A

changes in an atoms nucleus

43
Q

nuclear reaction

A

when atoms of one element change into another element in the nucleus

44
Q

strong nuclear force

A

attraction between nuclear particles that are close together (pushing inward force)

45
Q

nuclear particles

A

protons and nuetrons

46
Q

electrostatic force

A

repulsion between like charges (protons)

47
Q

how do strong nuclear force and electrostatic force act with eachother

A

they act against eachother

48
Q

nuclear stability
-what determines it

A

the size of the nucleus and ratio of neutrons to protons in the nucleus determines the stability

only unstable nuclei undergo nuclear reactions

if unstable electrostatic force will be greater than strong nuclear force

49
Q

isotopes - nuclear reactions

A

not all isotopes are able to undergo nuclear reactions

50
Q

radioactive isotopes

A

isotopes that are unstable

undergo nuclear decay to gain stability

51
Q

radiation
-types

A

energy and particles that are emitted by radioactive atoms

alpha particles, beta particles, x-rays, gamma rays

52
Q

alpha particles

A

can go to a persons hand

53
Q

beta particles

A

can go through a persons hand and to aluminum

54
Q

x-rays/gamma

A

can go through a persons hand, aluminum, and to lead

55
Q

isotopes - half lives

A

different isotopes have different half-lives

shorter half-life : decays quickly doesn’t remain in the environment for long

longer half life : decays slowly, remains in environment / body for a long time

56
Q

fission

A

when unstable nuclei are hit with a neutron

nucleus breaks up / falls apart into other nuclei

releases lots of energy

causes a chain reaction

if controlled can be useful

57
Q

what does the reactor vessel have

A

contains uranium

58
Q

what does the steam generator do

A

turns water to water vapor/steam

59
Q

what does the turbine do

A

uses speed / spins the steam

60
Q

what does the generator do

A

generates electricity with the steam

61
Q

what do the control rods do

A

control the rate of reaction / absorbs neutrons

62
Q

what does the condenser do

A

turns water vapor to water

63
Q

groups

A

columns (up and down)

determines family

64
Q

periods

A

rows (side to side)

represents number of rings

65
Q

dimitry mendeleev

A

first periodic table

organized by mass

predicted undiscovered elements

66
Q

periodic law

A

repetiton of chemical and physical properties of elements when arranged by increasing atomic number

67
Q

what family is group 1

A

alkali metals

brittle, corrodes quickly, gives off hydrogen in water

68
Q

what family is group 2

A

alkaline earth metals

69
Q

what family is groups 3-12

A

transition metals

70
Q

what family is group 17

A

halogens

different reactions to each other, produces white soils

71
Q

what family is group 18

A

noble gasses

72
Q

neutral atom

A

the # of protons = # of electrons

mass = protons + neutrons

EX:
Iodine (126.9)
protons: 53
electrons: 53
neutrons: 74 (Rounded atomic num - protons)

73
Q

atomic number

A

of protons in nucleus

defines an element

74
Q

average atomic mass

A

weighted average of all naturally occurring isotopes

does not equal the mass number

75
Q

average mass formula

A

[(mass) x (%abundance)] + [(mass) x (%abundance)]

always move decimal two places left for abundance percent before calculating

76
Q

metals

A

left side of the periodic table

excludes hydrogen

shiny, ductile, good conductors, malleable

ex: copper, gold, mercury

77
Q

where are nonmetals found

A

right side of the periodic table

includes hydrogen

no luster, various colors, brittle, poor conductors

ex: oxygen, chlorine, argon

78
Q

metalloids / semimetals

A

elements that line the staircase

-boron
-silicon
-germanium
-arsenic
-antimony (sb)
-tellurium
-polonium

79
Q

nuclear notation

A

(mass / protons + neutrons)
symbol
(atomic number / protons)

80
Q

three things the periodic table is organized by

A

-atomic number / # of protons

-family

-metals, nonmetals, metalloids

81
Q

elements in the same group all have the same number of _______

A

valence electrons

82
Q

elements in the same period all have the same number of _____

A

rings

83
Q

percent remaining formula

A

new percent
—————— x 100 = percent
old percent

berlin b (4 decks)

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