Chapter 5-6 Flashcards Preview

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Flashcards in Chapter 5-6 Deck (73):
1

was the first to discover some elements had similar properties (early 1800's) --

Johann Doberiener

2

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

Johann Doberiener

3

he organized elements in order of increasing mass -

John Newlands

4

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

John Newlands

5

1-7 elements =

different properties

6

8th element =

property like element 1

7

9th element =

property like element 2

8

repeating patterns ..

octaves

9

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

Dmitri Mendeleev

10

he organized the 1st periodic table =

Dmitri Mendeleev

11

he worked under Rutherford

Henry Moseley

12

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

Henry Moseley

13

he organized elements by atomic #, not mass # =

Henry Moseley

14

how many elements are there?

117 elements

15

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

group

16

elements in a row
numbered by energy levels, starting at the top

period

17

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

increase
elements

18

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

because it was to hard

19

they're silver-gray, except copper & gold

metals

20

they're also called semimetals =

metalloids

21

they have high melting points -

metals

22

they don't reflect light =

non-metals

23

they DO reflect light when polished -

metals

24

they are poor conductors of heat and electricity -

non-metals

25

they can be bent / hammered flat -

metals

26

they are good conducters of heat and electricity -

metals

27

they are properties of metals and nonmetals

metalloids

28

"silicon valley" =

metalloids

29

materials that engineers work w/

metalloids

30

brittle, low melting points -

non-metals

31

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

non-metals

32

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

valence elevtrons

33

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

valence electrons

34

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

ones place

35

the # of valence electrons varies for what blocks?

the d & f blocks

36

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

periodic law

37

systematic means ...

order

38

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

periodic trend

39

all atoms on the same energy level -

atomic radius

40

left to right (electrons get pulled in) -

atomic radius

41

it ____________ from left to right. -

decreases

42

why does it decrease from left to right -

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

43

they pull on all electrons -

protons

44

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

protons
pulled

45

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

pull
necleus

46

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

harder to take away

47

electrons w/ less energy & NOT close =

easy to take away

48

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

^^ what is this called =

Ionization Energy

49

small radius = close electrons = harder to take away =

higer energy

50

large radius = far electrons = easy to take away =

low energy

51

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

electronegativitiy

52

low electronegativity =

DOESNT want to take electron away

53

high electronegativity =

DOES want to take electron away

54

high ionization energy = high elctronegativity which =

it takes

55

low ionization energy = low electronegativity which =

it gives

56

bigger atoms - electrons farther from nucleus =

less energy

57

all elements in a single group share .....

same properties

58

the properties of metalloids are ...

they are halfway between metals and non-metals

59

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

periodic law

60

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

electronegativity

61

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

ionization energy

62

when moving left to right the ......

atomic radius decreases

63

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

rare earth metals

64

distance between the nucleus of an atom to the outtermost part

atomic radius

65

whats another name for group 2 -

alicine earth metals

66

groups 18 also knows as ...

nobel gas

67

group 1 also known as ....

alkaline metals

68

what is the d block also known as ...

transition metals

69

group 1 also known as ...

alkali metals

70

group 17 also known as ...

halogens

71

where are metalloids?

the ziggy line on periodic table

72

where are metals?

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

73

where are non-metals =

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