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Honors Biology 1 > Chemistry Ms19-25 > Flashcards

Chemistry Ms19-25 Flashcards

(97 cards)

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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
an atom is mostly made up of what?
space
26
how many e- can fit in an orbital?
2
27
changing an atoms number of protons =
a different element
28
changing an atoms number of neutrons =
isotope
29
changing the number of electrons =
ion
30
what is a cation
positive
31
what is an anion
negative
32
what is Thomson's plumb pudding model do?
hypothesis about atomic structure
33
what is Rutherford's gold foil experiment?
hypothesis that an atom is mostly space
34
what do columns share on the periodic table?
the same number of valence shell e-
35
what are rows arranged by?
energy levels
36
how are energy levels filled?
lowest first
37
how are S orbitals shaped and how many are there per energy level?
spherically shaped, 1 per energy level
38
how are P orbitals shaped and how many are there per energy level?
dumbbell shape, 3 per energy level
39
how are D orbitals shaped and how many are there per energy level?
clover shaped, 5 per energy level
40
when are there S P and D orbitals?
energy level >= 4
41
what is the max number of electrons per energy level when n> 2
18 electrons
42
how do orbitals filled?
sequentially; lowest to highest
43
n^2 =?
of orbitals per energy level
44
2n^2= (2)
of electrons per energy level
45
the octet rule?
atoms like to fill S and P orbitals in order to try to achieve noble gas state
46
where are valence electrons found?
where the orbitals are the farthest out
47
what is the reactivity level of elements close to a noble gas configuration?
Highly reactive
48
what is the reactivity level of noble gases?
stable
49
what is Hund's rule?
electrons occupy orbitals singly before they pair, from left to right
50
what is a Lewis Dot Structure used for?
used to predict/show chemical bonds
51
what elements are in covalent bonds?
non-metal + non-metal
52
what elements are in ionic bonds?
metal + non-metal
53
what do covalent bonds produce?
molecules
54
what do ionic bonds produce?
salts
55
how do you break bonds?
absorption of energy
56
how do you from bonds?
release of energy
57
what is exothermic reactions?
a reaction that releases more energy than it absorbs
58
what is endothermic reactions?
a reaction that absorbs more energy than it releases
59
what is a mole
a unit of measurement for an amount of a substance
60
the number of atoms in a mole is the same but the ___ can vary
mass
61
Conversion chart for moles to grams?
grams of substance over moles of substance is equal to molar mass of the substance in grams over one mole
62
What is molar mass?
the sum of each atom's atomic mass
63
What operation do you use for g to mol? For mol to g?
g to mol is division while mol to g is multiplication
64
H2O is a very good medium for what?
chemical reactions
65
what percentage of cells are water?
70%
66
when do cells shutdown?
when water percentage is lower than 50%
67
what is a polar molecule?
e- shared unevenly across covalent bonds, resulting in partial charges at the poles of the molecule
68
what is electron negativity?
e- grabbing/hogging power of an atom (unbalanced)
69
what does electron negativity cause?
e- are pulled towards atoms w/higher electron negativity
70
when do you have no electronegativity?
with the same atom (&covalent bonds)
71
why is H2O bent?
H atoms are pushed away from O atom because of electron negativity
72
what charge does the atom(s) that is pulling the e- to it have
slightly -
73
what charge does the atom(s) that is having their e- pulled?
slightly +
74
what results in molecule to molecule attractions?
Polarity
75
what are hydrogen bonds in terms of power?
weak alone powerful together
76
what is the gas state of H2O like?
H bonds form/break quickly; molecules farther apart
77
what is the liquid state of H2O like?
denser than solid; H bonds form/break less quickly; molecules tightly packed together
78
what is the solid state of H2O like?
H bonds form in geometric pattern(crystal lattice), pattern results in larger spacing between molecules than liquid form; solid
79
what is molarity?
a unit of concentration
80
if you have higher molarity you have higher____?
concentration
81
how to find molarity chart?
molarity is equal to number of moles of solute divided by Liters of solute
82
H2O is a __ solvent?
universal
83
what does it mean that H2O is a universal solvent?
forms H bonds w/ other polar substances(salts)
84
what does a hydration shell form around, and what do they do?
forms around ions and other polar substances breaking solids down into individual molecules through dissolving
85
why does heat speed up dissolving?
because H20 molecules are moving quicker w/ a higher kinetic energy level
86
"solution" arrows
solvent---> solute-----> solution
87
what is solubility?
how well a substance dissolves in a solvent
88
what does water do (connections)?
adhesion and cohesion
89
what is adhesion
surface connection
90
what is cohesion
self connection (like)
91
what is the difference of water on a polar vs. non polar surface?
wide on polar; tight on non polar
92
what kind of bond is cohesion?
H bond
93
what does spherical curvature do?
maximizes H20 cohesion and adhesion
94
what is heat capacity?
amount of heat required to raise a substances temperature 1 degree celsius (H2O's is exceptionally high)
95
example of H20 heat capacity?
ocean. 80-90% of heat absorbed in ocean without significant rise in temperature
96
what are colligative properties? & example
amount of solutes dissolved in H20 alters its properties; antifreeze in water keeps it from freezing with a high concentration of solutes
97
what do fish produce to lower the freezing point of their blood?
proteins that dissolve into the blood

Honors Biology 1 (22 decks)

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