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Honors Biology 1 > Chemistry Ms19-25 > Flashcards

Chemistry Ms19-25 Flashcards

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1
Q

define atom

A

the smallest unit of matter

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2
Q

define atomic nucleus

A

where protons and neutrons are located

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3
Q

define electron

A

negatively charged subatomic particle known as “e-“; has negligible mass

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4
Q

define neutron

A

neutrally charged subatomic particles located in nucleus

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5
Q

define proton

A

positively charged subatomic particles located in nucleus

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6
Q

define orbital

A

path that e- follows

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7
Q

how to find Atomic Mass?

A

protons+neutrons

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8
Q

what are protons equal to?

A

atomic #

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9
Q

define valence shell

A

of the outer shells where electrons bond

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10
Q

where are higher energy levels?

A

higher energy levels are found farther from nucleus

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11
Q

what is matter?

A

has makes and takes up space

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12
Q

what is an element?

A

a pure substance made up of only one kind of atom with a characteristic number of protons

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13
Q

what is an isotope?

A

a variation on the the element that has the same number of protons but a different number of neutrons, changing its mass

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14
Q

what is an ion?

A

an atom that is positively (cation) or negatively charged(anion)

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15
Q

what is a molecule?

A

2 or more atoms covalently bonded together

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16
Q

what is a compound?

A

different atoms chemically bonded together

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17
Q

what is atomic mass?

A

of protons and neutrons in an atom

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18
Q

what is atomic #?

A

that tells us how many protons are in an atom

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19
Q

how do you find the number of protons in an element?

A

the atomic number is equal to the number of protons

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20
Q

find the number of e- in an element?

A

same as the number of protons

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21
Q

how do you calculate the number of neutrons in an element?

A

atomic mass - atomic number

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22
Q

how do you determine the number of e- in the valence shell?

A

use family number (column)

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23
Q

names of groups and elements?

A

alkaline earth, alkaline, transition, halogens, noble gases

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24
Q

which elements make up 96% of organic matter?

A

carbon, hydrogen, nitrogen, oxygen

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25
Q

an atom is mostly made up of what?

A

space

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26
Q

how many e- can fit in an orbital?

A

2

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27
Q

changing an atoms number of protons =

A

a different element

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28
Q

changing an atoms number of neutrons =

A

isotope

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29
Q

changing the number of electrons =

A

ion

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30
Q

what is a cation

A

positive

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31
Q

what is an anion

A

negative

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32
Q

what is Thomson’s plumb pudding model do?

A

hypothesis about atomic structure

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33
Q

what is Rutherford’s gold foil experiment?

A

hypothesis that an atom is mostly space

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34
Q

what do columns share on the periodic table?

A

the same number of valence shell e-

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35
Q

what are rows arranged by?

A

energy levels

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36
Q

how are energy levels filled?

A

lowest first

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37
Q

how are S orbitals shaped and how many are there per energy level?

A

spherically shaped, 1 per energy level

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38
Q

how are P orbitals shaped and how many are there per energy level?

A

dumbbell shape, 3 per energy level

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39
Q

how are D orbitals shaped and how many are there per energy level?

A

clover shaped, 5 per energy level

40
Q

when are there S P and D orbitals?

A

energy level >= 4

41
Q

what is the max number of electrons per energy level when n> 2

A

18 electrons

42
Q

how do orbitals filled?

A

sequentially; lowest to highest

43
Q

n^2 =?

A

of orbitals per energy level

44
Q

2n^2= (2)

A

of electrons per energy level

45
Q

the octet rule?

A

atoms like to fill S and P orbitals in order to try to achieve noble gas state

46
Q

where are valence electrons found?

A

where the orbitals are the farthest out

47
Q

what is the reactivity level of elements close to a noble gas configuration?

A

Highly reactive

48
Q

what is the reactivity level of noble gases?

A

stable

49
Q

what is Hund’s rule?

A

electrons occupy orbitals singly before they pair, from left to right

50
Q

what is a Lewis Dot Structure used for?

A

used to predict/show chemical bonds

51
Q

what elements are in covalent bonds?

A

non-metal + non-metal

52
Q

what elements are in ionic bonds?

A

metal + non-metal

53
Q

what do covalent bonds produce?

A

molecules

54
Q

what do ionic bonds produce?

A

salts

55
Q

how do you break bonds?

A

absorption of energy

56
Q

how do you from bonds?

A

release of energy

57
Q

what is exothermic reactions?

A

a reaction that releases more energy than it absorbs

58
Q

what is endothermic reactions?

A

a reaction that absorbs more energy than it releases

59
Q

what is a mole

A

a unit of measurement for an amount of a substance

60
Q

the number of atoms in a mole is the same but the ___ can vary

A

mass

61
Q

Conversion chart for moles to grams?

A

grams of substance over moles of substance is equal to molar mass of the substance in grams over one mole

62
Q

What is molar mass?

A

the sum of each atom’s atomic mass

63
Q

What operation do you use for g to mol? For mol to g?

A

g to mol is division while mol to g is multiplication

64
Q

H2O is a very good medium for what?

A

chemical reactions

65
Q

what percentage of cells are water?

A

70%

66
Q

when do cells shutdown?

A

when water percentage is lower than 50%

67
Q

what is a polar molecule?

A

e- shared unevenly across covalent bonds, resulting in partial charges at the poles of the molecule

68
Q

what is electron negativity?

A

e- grabbing/hogging power of an atom (unbalanced)

69
Q

what does electron negativity cause?

A

e- are pulled towards atoms w/higher electron negativity

70
Q

when do you have no electronegativity?

A

with the same atom (&covalent bonds)

71
Q

why is H2O bent?

A

H atoms are pushed away from O atom because of electron negativity

72
Q

what charge does the atom(s) that is pulling the e- to it have

A

slightly -

73
Q

what charge does the atom(s) that is having their e- pulled?

A

slightly +

74
Q

what results in molecule to molecule attractions?

A

Polarity

75
Q

what are hydrogen bonds in terms of power?

A

weak alone powerful together

76
Q

what is the gas state of H2O like?

A

H bonds form/break quickly; molecules farther apart

77
Q

what is the liquid state of H2O like?

A

denser than solid; H bonds form/break less quickly; molecules tightly packed together

78
Q

what is the solid state of H2O like?

A

H bonds form in geometric pattern(crystal lattice), pattern results in larger spacing between molecules than liquid form; solid

79
Q

what is molarity?

A

a unit of concentration

80
Q

if you have higher molarity you have higher____?

A

concentration

81
Q

how to find molarity chart?

A

molarity is equal to number of moles of solute divided by Liters of solute

82
Q

H2O is a __ solvent?

A

universal

83
Q

what does it mean that H2O is a universal solvent?

A

forms H bonds w/ other polar substances(salts)

84
Q

what does a hydration shell form around, and what do they do?

A

forms around ions and other polar substances breaking solids down into individual molecules through dissolving

85
Q

why does heat speed up dissolving?

A

because H20 molecules are moving quicker w/ a higher kinetic energy level

86
Q

“solution” arrows

A

solvent—> solute—–> solution

87
Q

what is solubility?

A

how well a substance dissolves in a solvent

88
Q

what does water do (connections)?

A

adhesion and cohesion

89
Q

what is adhesion

A

surface connection

90
Q

what is cohesion

A

self connection (like)

91
Q

what is the difference of water on a polar vs. non polar surface?

A

wide on polar; tight on non polar

92
Q

what kind of bond is cohesion?

A

H bond

93
Q

what does spherical curvature do?

A

maximizes H20 cohesion and adhesion

94
Q

what is heat capacity?

A

amount of heat required to raise a substances temperature 1 degree celsius (H2O’s is exceptionally high)

95
Q

example of H20 heat capacity?

A

ocean. 80-90% of heat absorbed in ocean without significant rise in temperature

96
Q

what are colligative properties? & example

A

amount of solutes dissolved in H20 alters its properties; antifreeze in water keeps it from freezing with a high concentration of solutes

97
Q

what do fish produce to lower the freezing point of their blood?

A

proteins that dissolve into the blood

Honors Biology 1 (22 decks)

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