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chapter 1 Flashcards

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1
Q

central science, aka

A

chemistry

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2
Q

what does iupac stand for

A

lnternational union of pure and applied chemistry

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3
Q

first atomic theory

A

the greeks

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4
Q

who discovered matter can be subdivided into indivisible particles

A

greeks

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5
Q

democritus discovered what

A

different sizes, constant motions, empty space around them

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6
Q

who helped develop modern glassware

A

the alchemists (fULL METAL ALCHEMISTSSSS)

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7
Q

who discovered that matter was composed of earth, air, water, fire

A

aristotle (AND DANTEEEE)

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8
Q

___’s Atomic Theory

A

Dalton

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9
Q

who created the plum pudding model (ew everything just floating around ik there)

A

JJ Thompson

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10
Q

who directed alpha particles research

A

rutherford (my boyyy)

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11
Q

chadwick (:’l) did what

A

confirmed presence of neutrons

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12
Q

who revised the planetary model and showed that electrons release bursts of light when absorbing energy

A

bohr

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13
Q

a
E (what is E?)
z

A

chemical symbol of element

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14
Q

a
E (what is a?)
z

A

mass number

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15
Q

what is mass number

A

protons and neutrons

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16
Q

a
E (what is z?)
z

A

atomic number

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17
Q

what is atomic number

A

protons in nucleus

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18
Q

if an element has a full valence shell, it is

A

stable

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19
Q

how many valence electrons does helium have

A

2

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20
Q

which elements have a stable valence shell

A

noble gases

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21
Q

unstable elements want to be

A

stable

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22
Q

octet rule

A

elements combine with other atoms to attain a stable electron arrangement

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23
Q

when atoms lose or gain electrons, what is formed

A

an ion

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24
Q

cations are

A

positive

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25
Q

anions are

A

negative

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26
Q

metals tend to

A

LOSE valence electrons (they have few electrons in shell)

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27
Q

non metals tend to

A

gain electrons

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28
Q

element that can form more than one possible ion

A

multivalent ions

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29
Q

transition metals are commonly

A

multivalent

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30
Q

ion with more than one atom that acts as a single entity

A

polyatomic ion

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31
Q

examples of polyatomic ions

A

ammonium, NH4+

32
Q

ion in the human body

A

Na+

33
Q

atoms of same element with different numbers of neutrons

A

isotopes

34
Q

how to distinguish isotopes

A

mass number

35
Q

percentage of isotope in sample of element

A

isotopic abundance

36
Q

weighted average of masses of all isotopes of an element

A

atomic mass

37
Q

atomic mass formula

A

%abundance isotope (mass) + %abundance isotope (mass

38
Q

some isotopes are stable, while others

A

break apart easily (radioactive substances)

39
Q

when isotopes decay, they emit

A

nuclear radiation (in tiny particles)

40
Q

radiation=> alpha particles, beta particles, gamma particles

A

blocked by paper, blocked by aluminum, can penetrate most

41
Q

isotopes that produce nuclear radiation are called (lol)

A

radioisotopes

42
Q

alpha particle has the same structure as

A

He-4 nucleus, and a charge of 2+

43
Q

beta particle

A

negatively charged electron

44
Q

gamma ray

A

high energy electromagnetic radiation (no mass, speed of light)

45
Q

nuclear reaction

A

change in nucleus of atoms from presence of radioisotopes

46
Q

radioisotopes have a nucleus which can decay, releasing

A

energy and subatomic particles spontaneously

47
Q

in balancing nuclear reactions, the sum of mass numbers must be

A

equal on each side

48
Q

in balancing nuclear reactions, the sun of atomic numbers must

A

balance on each side

49
Q

alpha decay steps

A
  1. find alpha particle
  2. calculate atomic number and mass of new element
  3. find new element by looking up its atomic number
50
Q

alpha decay:

  1. 4
    Ra => He
  2. 2
A

226-4 and 88-2 is 222 and 86, Rn

51
Q

majority of known elements are

A

metals

52
Q

metals are

A

all solid except for mercury

53
Q

non metals (right of staircase)

A

non conductors
gas or solid
solids r brittle and matte

54
Q

metalloids (along staircase)

A

properties of metals and no metals

55
Q

Alkali, Akaline, Halogen, Noble Gases, Transition

A

AAHNT
wide range of properties
strong metals
high melting points
conductors
multivalent ions

56
Q

energy levels:

A

higher are more distant from nucleus

57
Q

charge on nucleus:

A

more charge pulls electrons in closer (positive and negative attract)

58
Q

shielding effect:

A

inner electrons repel outer electrons

59
Q

atomic and ionic radius

A

centre of atom to outermost electron

60
Q

ENC

A

effective nuclear charge

61
Q

down a group,

A

ENC decreases (adding orbits = increase distance of radius, inner electrons shield outer ones from nucleus charge)

outer electrons have a decreased attraction to nucleus, radius increases

62
Q

right across a period

A

ENC increases (increasing +ve charge, electrons added to same energy level, no electron shielding)

more attraction to nucleus, outer electrons pull closer, radius decreases

63
Q

ionic radius

A

size of ion compared to its atom

64
Q

cations, ENC

A

increases (nucleus pulls each electron closer, radius decreases)

65
Q

anions, ENC

A

decreases, shared among more electrons in anions

attraction is weaker on each electron, radius increases

66
Q

ionization energy

A

energy needed to remove an electron from neutral atom

67
Q

move down a group, ionization energy

A

decreases (the farther from nucleus, the easier to remove it)

68
Q

move right across a period, ionization

A

increases, atoms are smaller, nucleus pulls valence electrons

69
Q

down a group, attraction to nucleus goes down as atomic radius

A

increases (enc decreases)

70
Q

the further away from the nucleus, the

A

easier an electron can be removed with less energy

71
Q

right across a period, attraction increases as atomic radius

A

decreaes, (enc increases) (harder to remove electrons)

72
Q

noble gases have the highest

A

ionization energy of their period

73
Q

electron affinity

A

ability of an atom to gain electrons

74
Q

down a group, there is weak attraction to nucleus , electron affinity

A

decreases

75
Q

right across a period, atomic radius decreases, ENC increases, attraction to nucleus is

A

high

76
Q

down a group,

A

atomic radius increases
ie decreases
electron affinity decreases
electronegativity decreases or stays

77
Q

right across a period,

A

atomic radius decreases
ie increases
electron affinity increases
electronegativity increases

chem (7 decks)

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