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chem exam Flashcards

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1
Q

Metallic bond

A

M, M

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2
Q

Covalent bond

A

NM, NM

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3
Q

Ionic bond

A

NM, M

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4
Q

when naming formulas that are ionic

A

you don’t add prefixes

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5
Q

when naming formulas that are covalent

A

you add prefixes

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6
Q

significant figures steps
Ex. 34.50g and 3450g

A
  1. identify Pacific Atlantic
    Pacific - decimal Points, read from the left
    Atlantic- no points, read from the right
  2. Count #’s from either left or right
    0’s after # are counted, 0’s before # are not.
    Ex. 34.50g, 4 sig fig. 3450g 3 sig fig
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7
Q

Atom map: protons
center, first ring (VERY close to center NOT option A), second outer ring, floppy bags

A

center

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8
Q

Atom map: nuetrons
center, first ring (VERY close to center NOT option A), second outer ring, floppy bags

A

center

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9
Q

Atom map: valence electrons
center, first ring (VERY close to center NOT option A), second outer ring, floppy bags

A

very outer ring

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10
Q

Atom map: first s orbital
center, first ring (VERY close to center NOT option A), second outer ring, floppy bags

A

very closest ring

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11
Q

Atom map: p orbital
center, first ring (VERY close to center NOT option A), second outer ring, floppy bags

A

floppy bags

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12
Q

top left on periodic table

A

proton + nuetron

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13
Q

bottom on periodic table

A

nuetron

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14
Q

top left - bottom =

A

electron

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15
Q

atomic mass
ex. ^65 29Cu natural abundance 30.83% and ^63 29Cu natural abundance 69.17%

A

multiple top left x natural abundance (but move decimal 2x to the left for NA) + top left2 x NA 2
(65 x .3083) + (63 x .6917)

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16
Q

lewis dot diagram!!

A

follow the columns for the amount of dots, max 10 per orbital tho. max any at all is 18
ex. 5–> column 5 or column 15

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17
Q

BOHR model steps
Ex. ^16 32.06 S

A
  1. ^16- protons, 32.06- protons and neutrons, b/c charge is neutral means protons and nuetrons are equal
  2. put P^+ = 16 nd N* = 16, circle with an orbital and put 2 dots on it, 2nd orbital 8 dots, third 6 dots. (max 8 dots per orbital)
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18
Q

orbital box (arrows)

A

1s__ 2s__ 2p__
just calculate how many electrons and see how many left
^16- 32.06

19
Q

electron configuration (1s^2)
Neon 10

A

1s^2 1s^2 2p^6
just calculate how many electrons and see how many left
20-10

20
Q

Democritus

A

first to conceptualize the existence of atoms (was like everything is made of atoms!)

21
Q

JJ Thompson

A

developed plum pudding model

22
Q

Rutherford

A

disproved ppm with golden foil experiment

23
Q

Bohr

A

invented the Bohr diagram

24
Q

Schrodinger

A

published quantum mechanical model, quantum particles + waves

25
Q

nuclear equation
ex. ^232 90 Th–> ^228 88 Ra + ^A B C

A

^232- ^228 = A
90-88= B
^A B X, X=C
A=4 B=2 C=H

26
Q

types of decay:
Alpha decay

A

nuclear equation is 4/2

27
Q

types of decay:
Beta decay

A

nuclear equation has -1

28
Q

types of decay:
Gamma decay

A

nuclear equation has 0

29
Q

periodic table

A

increasing EN and ionization upward left
increasing EN and ionization going right top
increasing atomic radius right ownward

30
Q

define electronegativity

A

the attraction of an atom w/in a bond

31
Q

define atomic radii

A

the distance between the nucleus and valance electrons

32
Q

define ionization energy

A

the energy necessary to remove one electron

33
Q

sort from most to least electronegative

A

in order of distance from upper right corner of pd

34
Q

covalent electrons

A

shares valence electrons

35
Q

ionic electrons

A

NM take valence electrons from the M

36
Q

metallic electrons

A

an electron sea

37
Q

metallic conductors

A

great conductors

38
Q

ionic conductors

A

alr conductors

39
Q

covalent conductors

A

bad conductors
good insulator

40
Q

what’s bond angle H2O

A

104.5

41
Q

number naming

A

mon di tri tetra

42
Q

Naming ray

A

D and B

43
Q

types of reactions

A

combustion, double replacement, single replacement, synthesis

44
Q
A

driving ed :) (24 decks)

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