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chemistry > chapter 6: periodic table > Flashcards

chapter 6: periodic table Flashcards

1
Q

How is the periodic table organized?

A

By properties

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2
Q

Who was Dmitri Mendeleev?

A

A Russian chemist and teacher

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3
Q

Why is Dmitri Mendeleev important?

A

Made the first periodic table

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4
Q

How did Dmitri Mendeleev arrange the periodic table?

A
  • Arranged elements in order of increasing atomic mass
  • He left blanks for yet undiscovered elements
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5
Q

What did Henry Moseley do in 1913?

A

Arranged elements according to increasing atomic number on periodic table

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6
Q

Who’s table is used today, Mendeleev or Moseley?

A

Moseley

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7
Q

What is a group or family?

A

Vertical (down) rows on periodic table

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8
Q

What is a period?

A

Horizontal rows on periodic table

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9
Q

How many periods are on the periodic table?

A

7

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10
Q

How many groups/families are on the periodic table?

A

18

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11
Q

Reactivity increases/decreases as you go up/down?

A

increases as you go down

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12
Q

1st group

A

alkaline metals

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13
Q

2nd group

A

alkaline earth metals

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14
Q

3rd-12th group

A

transition metals

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15
Q

13th group

A

boron

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16
Q

14th group

A

carbon

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17
Q

15th group

A

nitrogen

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18
Q

16th group

A

oxygen or chalcogens

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19
Q

17th group

A

halogens

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20
Q

18th group

A

noble gasses

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21
Q

F block

A

inner transition metals

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22
Q

What is the periodic law?

A

When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

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23
Q

Where are metals on the periodic table?

A

to the left (everything under metalloids)

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24
Q

Where are non-metals on the periodic table?

A

Hydrogen and everything up from metalloids

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25
Q

Where are metalloids on the periodic table

A

B, Si, Ge, As, Sb, Te, Po

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26
Q

Metals are…

A

electrical conductors, have luster, ductile, malleable

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27
Q

Non-metals are…

A

generally brittle and non-lustrous, poor conductors of heat and electricity

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28
Q

Metalloids are…

A

Properties are intermediate between metals and nonmetals

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29
Q

Alkaline metals are…

A

Extremely reactive

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30
Q

What is Atomic Radius/Size?

A

increases down the group and decreases from left to right across the period

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31
Q

What is Ionization Energy?

A

energy needed to remove an electron

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32
Q

Exceptions with IE

A

drops between 2nd-13th group and 15th-16th group

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33
Q

Drop between Be and B

A
  • Be is fully filled in s block meaning its stable and less likely to give an electron
  • B is less than half filled; ⅙ of p block so its unstable
34
Q

Which atoms have the highest and lowest IE?

A
  • H has the highest
  • Fr has the lowest
35
Q

What is Electronegativity?

A

force of attraction of one atom to another atoms electrons

36
Q

What is Electronafinity?

A

the amount of energy released when an atom accepts and electron

37
Q

What group has the highest electronafinity?

38
Q

Nuclear charge =???

A

number of protons - number of inner electrons

39
Q

Why does IE decrease?

A

Radius and shielding increases

40
Q

Which group tends to form 1+ ions?

A

Alkali metals

41
Q

Which group tends to form 2+ ions?

A

Alkali earth metals

42
Q

Which group tends not to form ions or react?

A

Noble gases

43
Q

How does the periodic table account for the pattern of IE?

A

Atoms have more protons and more pull on electrons across a period and more shells or energy levels and weaker pull on electrons down a group.

44
Q

The size of an element’s atomic radius __________ from left to right across the periodic table.

45
Q

The halogens tend to form anions because….

A

They are each only one electron away from having a full outer shell

46
Q

Name the only element touching the stair-step line that is NOT a metalloid

47
Q

When a metal atom becomes a cation…

A

Its ionic radius is smaller than its atomic radius

48
Q

Mendeleev left spaces in his periodic table and predicted several elements and their…

A

Properties

49
Q

Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing

A

Atomic mass

50
Q

Moseley’s work led to the realization that elements with similar properties occurred at regular intervals when the elements were arranged in order of increasing

A

atomic number

51
Q

Who used his experimental evidence to determine the order of the elements according to atomic number?

52
Q

The most useful source of general information about the elements for anyone associated with chemistry is a…

A

Periodic table

53
Q

The periodic table…

A

Permits the properties of an element to be predicted before the element is discovered.

54
Q

Evidence gathered since Mendeleev's time indicates that a better arrangement than atomic mass for elements in the periodic table is an arrangement by

A

Atomic number

55
Q

What are the radioactive elements with atomic numbers from 90 to 103 in the periodic table called?

56
Q

Argon, krypton, and xenon are

A

Noble gasses

57
Q

Which two periods have the same number of elements?

58
Q

The discovery of the noble gases changed Mendeleev’s periodic table by adding a new

59
Q

The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic

60
Q

Elements in a group or column in the periodic table can be expected to have similar

A

properties

61
Q

For groups 1, 2, and 18, the atomic number of the fourth element in the group is ____ more than the preceding element.

62
Q

Krypton, atomic number 36, is the fourth element in Group 18. What is the atomic number of xenon, the fifth element in Group 18?

63
Q

Identify the sublevels in a period that contains 32 elements.

A

s, p, d, f

64
Q

How many elements are in a period in which only the s and p sublevels are filled?

65
Q

The length of each period in the periodic table is determined by the

A

sublevels being filled with electrons.

66
Q

In Period 3 there are 8 elements. What sublevel(s) is (are) being filled?

67
Q

Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel?

68
Q

The period of an element can be determined from its

A

electron configuration

69
Q

Elements to the right side of the periodic table (p-block elements) have properties most associated with

70
Q

Elements in which the d-sublevel is being filled have the properties of

71
Q

The elements that border the zigzag line in the periodic table are

A

metalloids

72
Q

The group of 14 elements in the sixth period that have occupied 4f orbitals is the

A

Lanthanides

73
Q

For Groups 13 through 18, the total number of electrons in the highest occupied level equals the group number

74
Q

Periods with occupied f sublevels

A

are not assigned group numbers

75
Q

In nature, the alkali metals occur as

76
Q

atomic radius

A

increases as you go down; and decreases as you go left to right

77
Q

IE

A

decreases as you go down; increases as you go right

78
Q

Electronafinity

A

decreases as you go down; increases as you go right

79
Q

electronegativity

A

decreases as you go down; increases as you go right

80
Q

positive ion

81
Q

negative ion

chemistry (6 decks)

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