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Chemistry > Formulas + ch3 pp cont > Flashcards

Formulas + ch3 pp cont Flashcards

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1
Q

celsius to fahreinheit

A

oC = (oF-32)/1.8

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2
Q

celsius to kelvin

A

K = oC + 273

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3
Q

volume of a cube

A

Length L

V = L ^ 3

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4
Q

volume of a rectangular solid

A

Length L, width W, height H

V = L x W x H

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5
Q

volume of a cylinder

A

diameter D, height H

v = (πD^2H)/4 = (3.14D^2H)/4

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6
Q

Density of substance

A 
Density = Mass of substance g/ volume of substance m
D = M/V
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7
Q

fahreinheit to Celsius

A

oF = 1.8(oC) + 32

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8
Q

observed mass formula

A

Atomic weight1 amu x %
+ Atomic weight2 amu x %
_________________________
weighted average mass amu

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9
Q

electrons

A

subatomic particles that move around the other part of an atom

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10
Q

when atoms interact with one another what are the subatomic particles that participates in the interaction?

A

electrons

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11
Q

chemical properties of an atom, which are the basis for its identification are determined by?

A

the number and arrangement of electrons surrounding the nucleus

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12
Q

the atom is characterized by its atomic number or number of protons why?

A

because it has the same number of electrons and protons

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13
Q

ions

A

charged atoms

- charged particles

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14
Q

atoms acquire a charge by?

A
  • gaining or losing electrons
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15
Q

anoins

A
  • when atoms gain electrons

- become negatively charged ions

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16
Q

cations

A
  • when atoms lose electrons

- become positively charged ions

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17
Q

ions behave much differently than the neutral atoms

A
  • metal sodium - natural Na atom is highly reactive and unstable
  • sodium cations, Na+ - non reactive and stable (salt table)
  • since material like table salt are neutral - must be equal amounts of charge2 from cations and anions in them
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18
Q

subatomic structure of ions

- protons

A

protons are never changed during chemical reactions

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19
Q

orbitals

A
  • space where electron occupies and move around in

- divided by shells and subshell

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20
Q

location and shape of an orbital is defined by?

A

shell and subshell

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21
Q

shell

A

layer of space surrounding the nucleus, just like an onion shell

  • each shell is designated by an integer, called quantum number (n= 1,2,3,4…)
  • Shell #1 closest to the nucleus - number increases - distance of shell from nucleus does as well
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22
Q

subshell

A
  • specific shape of space within a shell
  • designated by alphabet letters
  • s shere
  • p 2 lobed hourglass
  • d 4 lobed clover leave
  • f 8 lobed space
23
Q

n = 1 shell

A
  • 1 subshell

- s

24
Q

n= 2 shell

A

2 subshell

- s p

25
Q

n = 3 shell

A
  • 3 subshell

- s p d

26
Q

n = 4 shell

A
  • 4 subshells

- s p d f

27
Q

the energy of an electron depends on?

A

the energy of the subshell it occupies

28
Q

energy of a subshell is determined by?

A

the shell # and its shape (type of subshell)

29
Q

what is the most important determinant for the energy of an orbital?

A

the shell #

30
Q

the higher the shell number?

A
  • the farther the shell is from the nucleus

- the higher the energy level

31
Q

since shell number determines the energy level of an electron in the shell, the shell is also called?

A

an energy “level”

32
Q

sublevel

A
  • subshell

- energy of the subshell increases with the complexity of its shape

33
Q

orbitals capacity for electrons

A
  • each orbital can hold up to 2 electrons

- contains two electrons that must spin in opposite direction

34
Q

rules for filling electrons in orbitals

A
  1. atoms always fill their lowest energy orbitals first and successively higher ones as more electrons are added - aufbau principle
  2. each orbital can only have 2 electrons (pauli exclusion principle)
  3. electrons fill unoccupied orbitals within a subshell first before filling singularly-occupied ones (hunds rule)
35
Q

core electrons

A

electrons in the inner filled shells

- have low energy and are extra stable

36
Q

valence

A

electrons are electrons in the outermost shell, or electrons in the shell with the highest shell number
- involved in chem reactions

37
Q

valence electrons of an element vs its location on the periodic table

A
  1. element in same group has same number of valence electrons
  2. group A # = total # of valence electron
  3. period # = shell # of the valence electron
38
Q

elements filling the 4s subshell

A

Group 1A, alkaline metal - Ar
Group 2A, alkaline metal
K, Ca

39
Q

elements filling the 3d subshell

A
  • Grps B transition metals

Cu, Zn

40
Q

elements filling the 4p subshells

A

Groups 3A, 7A, and 8

Ga Ge Kr

41
Q

The # of columns in different part of the periodic table corresponds to?

A

the max electron capacity for each subshell type

42
Q

the column location of an element indicates?

A
  • the type of subshell filled by its highest energy electrons
43
Q

the column location of an element within a block indicates?

A

the # of the highest energy electrons in the specific type of subshell

44
Q

the period location of an element?

A

gives information about the shell number of its highest energy electrons

45
Q

of e =

A

atomic number

46
Q

each square in period table =

A

1 e-

47
Q

core

A

inert gas from the last period

48
Q

of core e- =

A

atomnic number of the core inert gas

49
Q

period n

energy level is n for?

A

e- in s and p block

50
Q

period n

energy level is n-1

A

for e- in d block

51
Q

period n

energy level is n-2 for

A

e- in f block

52
Q

sum of superscript =

A

atomic number

53
Q

metal lose e- anbd nonmetal gaining e- have same electron configuration as?

A

noble gases

Chemistry (17 decks)

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