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Copy - Chemistry 0569 > Chapter 5-6 > Flashcards

Chapter 5-6 Flashcards

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1
Q

was the first to discover some elements had similar properties (early 1800’s) –

A

Johann Doberiener

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2
Q

he also figured if you average mass of 3 elements, is the mass of the middle element -

A

Johann Doberiener

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3
Q

he organized elements in order of increasing mass -

A

John Newlands

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4
Q

he noticed that properties of the elements seem to repeat every 8 elements

A

John Newlands

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5
Q

1-7 elements =

A

different properties

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6
Q

8th element =

A

property like element 1

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7
Q

9th element =

A

property like element 2

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8
Q

repeating patterns ..

A

octaves

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9
Q

he wroter properties of each elements on cards & then arranged them in various ways =

A

Dmitri Mendeleev

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10
Q

he organized the 1st periodic table =

A

Dmitri Mendeleev

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11
Q

he worked under Rutherford

A

Henry Moseley

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12
Q

he used x-rays to assign each element a whole #, called the atomic # =

A

Henry Moseley

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13
Q

he organized elements by atomic #, not mass # =

A

Henry Moseley

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14
Q

how many elements are there?

A

117 elements

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15
Q

elements w/ similar properties
arranged in columns
numbered 1-18, starting at the left

A

group

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16
Q

elements in a row

numbered by energy levels, starting at the top

A

period

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17
Q

as the number ___________, so does the number of ___________ in the period.

A

increase

elements

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18
Q

why was the f-block taken out and put in the bottom =

A

because it was to hard

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19
Q

they’re silver-gray, except copper & gold

A

metals

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20
Q

they’re also called semimetals =

A

metalloids

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21
Q

they have high melting points -

A

metals

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22
Q

they don’t reflect light =

A

non-metals

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23
Q

they DO reflect light when polished -

A

metals

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24
Q

they are poor conductors of heat and electricity -

A

non-metals

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25
Q

they can be bent / hammered flat -

A

metals

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26
Q

they are good conducters of heat and electricity -

A

metals

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27
Q

they are properties of metals and nonmetals

A

metalloids

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28
Q

“silicon valley” =

A

metalloids

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29
Q

materials that engineers work w/

A

metalloids

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30
Q

brittle, low melting points -

A

non-metals

31
Q

they are mostly solid or gas at room temperature, except Br = liquid

A

non-metals

32
Q

they are the electrons in the highest energy level of an atom =

A

valence elevtrons

33
Q

they are the only electrons that can bond w/ another element to make compounds -

A

valence electrons

34
Q

to find the # of valence electrons, always used the _________ ________ of the group number.

A

ones place

35
Q

the # of valence electrons varies for what blocks?

A

the d & f blocks

36
Q

its when elements are arranged in order of increasing atomic number, their physcial and chemical properties show a periodic (repeating) pattern -

A

periodic law

37
Q

systematic means …

A

order

38
Q

systematic and predictable variation in a physcial or chemical property of each element as you move throught the periodic table =

A

periodic trend

39
Q

all atoms on the same energy level -

A

atomic radius

40
Q

left to right (electrons get pulled in) -

A

atomic radius

41
Q

it ____________ from left to right. -

A

decreases

42
Q

why does it decrease from left to right -

A

as you move to the right, each atom adds a proton & electron

43
Q

they pull on all electrons -

A

protons

44
Q

the more _______, the more the electrons get _______ on.

A

protons

pulled

45
Q

the more the protons _____, the closer the electrons are too the _________

A

pull

necleus

46
Q

the elctron w/ a lot of energy & is close=

A

harder to take away

47
Q

electrons w/ less energy & NOT close =

A

easy to take away

48
Q

the elctron w/ a lot of energy & is close
electrons w/ less energy & NOT close

^^ what is this called =

A

Ionization Energy

49
Q

small radius = close electrons = harder to take away =

A

higer energy

50
Q

large radius = far electrons = easy to take away =

A

low energy

51
Q

how much an atom wants to take an electron away from another atom =

A

electronegativitiy

52
Q

low electronegativity =

A

DOESNT want to take electron away

53
Q

high electronegativity =

A

DOES want to take electron away

54
Q

high ionization energy = high elctronegativity which =

A

it takes

55
Q

low ionization energy = low electronegativity which =

A

it gives

56
Q

bigger atoms - electrons farther from nucleus =

A

less energy

57
Q

all elements in a single group share …..

A

same properties

58
Q

the properties of metalloids are …

A

they are halfway between metals and non-metals

59
Q

the elements are arranged in order of increasing atomi c #; it shows a repeating pattern -

A

periodic law

60
Q

how much an atom wants to take away electrons from another -

A

electronegativity

61
Q

amount of energy it takes to remove an electron from an atom =

A

ionization energy

62
Q

when moving left to right the ……

A

atomic radius decreases

63
Q

what are the elements on the bottom of the periodic table called -

A

rare earth metals

64
Q

distance between the nucleus of an atom to the outtermost part

A

atomic radius

65
Q

whats another name for group 2 -

A

alicine earth metals

66
Q

groups 18 also knows as …

A

nobel gas

67
Q

group 1 also known as ….

A

alkaline metals

68
Q

what is the d block also known as …

A

transition metals

69
Q

group 1 also known as …

A

alkali metals

70
Q

group 17 also known as …

A

halogens

71
Q

where are metalloids?

A

the ziggy line on periodic table

72
Q

where are metals?

A

all the elements to the LEFT of the metalloids/ziggy line

73
Q

where are non-metals =

A

all the elementts to the left of the ziggy line/metalloids

Copy - Chemistry 0569 (22 decks)

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