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chem (dr nick) > Atoms > Flashcards

Atoms Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

Daltons atomic theory (4)

A

1) everything is made of atoms
2) atoms of the same element are identical, vice versa
3) atoms of diff elements combine in whole # ratios to make compounds
4) chemical reactions involve the rearrangements of atoms. no new atoms are created/destroyed

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2
Q

subatomic particles

A

proton, electron, neutron

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3
Q

charge of proton

A

+

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4
Q

charge of electron

A

-

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5
Q

charge of neutron

A

0

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6
Q

proton relative mass

A

1

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7
Q

electron relative mass

A

0

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8
Q

neutron relative mass

A

1

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9
Q

what is the atomic #

A

number of protons

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10
Q

what is the mass number

A

how many protons + neutrons

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11
Q

how many electrons are in an atom

A

same as # of protons

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12
Q

what is the charge of an atom?

A

0/neutral

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13
Q

what is an isotope

A

atoms with a diff number of neutrons and same number of protons

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14
Q

amu formula

A

avg = mass1(percentage1) +…

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15
Q

who is mendeleev

A

russian chemist who created the first periodic table

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16
Q

who is henry mosley

A

chemis who arranged periodic table to what we use today (increased atomic #)

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17
Q

why is the periodic table called the periodic table

A

because of the periodic repetition

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18
Q

what is a group/family

A

verticale rows of the periodic table

have similar reactions

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19
Q

what is a period

A

a horizontal row in the periodic table

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20
Q

what are metal

A
  • largest region
  • conduct heat/electricity
  • lustrous
    -malleable
    -ductile
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21
Q

what are metalloids

A
  • have properties of metals and nonmetals
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22
Q

what are noble gases

A

group 8 elements
-exist in gaseous state at normal temp and are non reactive with other metals

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23
Q

what are alkali metals

A

group 1 elements
-highly reactive

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24
Q

what are alkaline metals

A

group 2 elements

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25
Q

smallest particle of an element?

A

atom

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26
Q

what particles form the nucleus?

A

protons & neutrons

27
Q

how does the mass of a neutron compare to mass of a proton

A

basically the same, proton slightly heavier

28
Q

atoms of the same elements arent always identical because…

A

of isotopes

29
Q

what is the charge of the nucleus

A

positive

30
Q

how to write nuclear symbols

A

mass #
Element
atomic #

31
Q

what are halogens

A

non metals in period 17

32
Q

what are sig figs

A

include all of the digits that are known plus one more that is estimated

33
Q

rules for counting sig figs (4)

A

1) numbers other than 0 always count (ex. 3645 has 4 sig figs)
2) leading zeros do NOT count (ex. 0.0845 has 3 sig figs)
3) captive zeroes are always sig figs (ex. 16.07 has 4 sig figs)
4) trailing zeros are only sig figs if there’s a decimal point (ex. 2500.000 has 7 sig figs)

34
Q

special situations where there’s an unlimited amount of sig figs (2)

A

1) counted items (ex. 12 people or 425 thumbtacks)
2) exactly defined quantities

35
Q

how to convert grams

A

x1000 x1000
kg ———> grams———-> mg
<——— <———-
/1000 /1000

36
Q

how to convert meters

A

milli-meter = 1000mm for 1m
centi-meter= 100 cm for 1m

37
Q

density formula

A

d=m/v

38
Q

is density a physical or chemical property?

A

physical

39
Q

as density decreases, temperature…

A

increases

40
Q

what is matter

A

matter is anything that
1) has mass
2) has volume (takes up space)

41
Q

what are chemical properties

A

a property that can k my be observed by changing the composition of the material
(ex. flammability, decomposition, fermentation)

42
Q

what are physical properties

A

a property that can be observed and measured without changing the materials composition
(ex. color, hardness, melting & boiling points)

if you can reverse it, it’s a physical change

43
Q

who created the current periodic table

A

henry mosely

44
Q

who created the first periodic table

A

mendeleev

45
Q

what is an ion

A

a charged particle

46
Q

two types of ions

A

1) cation
2) anion

47
Q

what is a cation

A

ion with + charge

48
Q

what is an anion

A

ion with - charge

49
Q

what is electron configuration

A

ways elections are arranged in orbitals

50
Q

what are the rules of electron configuration (3)

A

1) aufbau principle: electrons enter the lowest energy level first
2) pauli principle: only 2 electrons per orbital
3) hunds rule: when electrons occupy orbital of equal energy

51
Q

what are unpaired electrons

A

an orbital with only one electron instead of 2

52
Q

what are valence electrons

A

the highest principle energy level

53
Q

what is the periodic trend for atomic size

A

increases as it goes ⬇️
increases as it goes ⬅️

54
Q

what ionization energy

A

ionization energy is the amount of energy it takes to completely remove and election from a gaseous atom

55
Q

what are the periodic trends for ionization

A

increases ⬆️
increases ➡️

56
Q

periodic trend of melting/boiling point

A

highest in the middle

57
Q

what is electronegativity

A

tendency for an atom to attract electrons to itself when combined with another atom

58
Q

what are the periodic trends for electronegativitiy’s size

A

increases ⬆️
increases ➡️

59
Q

what is empiricle formula

A

lowest whole number ratio of atoms in a compound

60
Q

what is molecular formula

A

the true number of atoms of each element

61
Q

how do you do molar conversions

A

mols x molar mass= mass
mols x 22.4 = volume
mols x 6.02 x 10^23= molecules

62
Q

what are ionic compounds

A

metal + another metal

63
Q

what are covalent compounds

A

metal + nonmetal

chem (dr nick) (4 decks)

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