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chemistry reading guides > Ch 5 Reading Guide > Flashcards

Ch 5 Reading Guide Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

The first chemist to organize elements according to their properties was who?

A

Dimitri Mendeleev

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2
Q

Dmitri placed the elements in a table according to ______ atomic masses

A

Increasing

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3
Q

Any repeating pattern is referred to as ______

A

Periodic

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4
Q

What did the blank spaces on demitri’s Chart represent?

A

Undiscovered elements

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5
Q

Moseley determined that the elements fit better on the periodic table if arranged according to increasing _______

A

Atomic number

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6
Q

The ______ law states that the physical and ______ properties of the elements are periodic functions of their ______ numbers

A

Periodic, chemical, atomic

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7
Q

The periodic table is an arrangement of elements in order of their atomic numbers so that elements with ____ properties fall in the same ______ or group

A

Similar, column

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8
Q

Which noble gas is a component of the sun?

A

Helium

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9
Q

List all of the noble gases

A

Helium, neon, argon, krypton, Xenon, radon

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10
Q

The ______ are the 14 elements atomic numbers 58 to 71

A

Lanthanides

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11
Q

The actinides are the 14 elements with atomic numbers from 90 to _______

A

103

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12
Q

The reason for periodicity is explained by the

________ Of electrons around the nucleus.

A

Arrangement

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13
Q

What is the group number of elements which undergo few chemical reactions?

A

18

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14
Q

Chemical properties of an element depend on the electron configuration of the ________ occupied energy level

A

Highest

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15
Q

A horizontal row of elements is also called a

_______

A

Period

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16
Q

How many elements are found in the second period?

A

Eight

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17
Q

The periodic table can be divided into _____

Blocks

A

Four

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18
Q

Which block contains the most chemically reactive metals?

A

s-block

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19
Q

Where are the alkali metals located?

A

Group 1

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20
Q

Describe the chemical properties of the alkali metals

A

Extremely reactive with air and moisture

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21
Q

Name two physical properties of alkali metals

A

Silver appearance and soft

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22
Q

How many electrons are in the highest occupied energy level for the alkali metals?

A

One

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23
Q

How must The alkali metals the stored?

Why?

A

In kerosene, to prevent reactions

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24
Q

The elements of group to our called the ______

Earth metals

A

Alkaline

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25
Q

Are the elements in group 2 more or less reactive than those in group one?

A

Less

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26
Q

Is hydrogen considered to be a member of group one?

A

No

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27
Q

Why is helium placed in group 18 instead of group 2?

A

Because it has a full outer energy level. it is chemically stable.

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28
Q

The _______ elements are also known as the D block elements

A

Transitional

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29
Q

Do all do you block elements contain the same number of outer Shell electron?

A

No

30
Q

Which of the D block elements are least reactive

A

Paladium platinum and gold

31
Q

The S block and the P block elements together I referred to as the ______elements

A

Main group

32
Q

Name the metalloids

A

Boron, Silicon, Germainium, Arsenic, antimony, tellurium

33
Q

The elements in group 17 are called _______

A

Halogens

34
Q

The halogens are the most reactive _______

A

Non-metals

35
Q

Why are the halogens so reactive?

A

They are one electron short

36
Q

What color is chlorine?

A

Yellowish green

37
Q

The elements with electrons down the 4f orbitals are called the ________

A

Lanthanides

38
Q

The ______ contain electrons filling the 5F orbitals

A

Actinides

39
Q

How many actinides occur Naturally?

A

4

40
Q

All actinides are _______

A

Radioactive

41
Q

One half the distance Between the nuclei Of identical atoms that are bonded together is a measure of the _______

A

Atomic radius

42
Q

As you move from left to right across the period of elements The atomic radii _______

A

Decreases

43
Q

Why does the atomic radii decrease as you move from left to right across A period of elements?

A

The positive charge of the nucleus increases

44
Q

The atomic radii _______ as you move down periodic table within a group

A

Increases

45
Q

Write an equation to show the of an electron from an atom.

A

A+ Energy –> A+ electron

46
Q

An atom or group of bonded atoms that has a positive or negative charge is an _____

A

Ion

47
Q

_______ Is the process that results in the formation of an ion

A

Ionization

48
Q

The energy required to remove one electron from a neutral atom of an element is the ____

A

Ionization energy

49
Q

Describe ionization energy values for elements in group one in group 18

A

Group 1: The lowest Group 18: The highest

50
Q

Moving from left to right across a period of elements deionization energy values generally _____

A

Increases

51
Q

Among the main group elements ionization energy values generally _____ down in the group.
Why?

A

Decrease; Because the electrons are in higher Energy levels

52
Q

The energy required to remove the second electron from an atom is always ______

A

Higher

53
Q

The energy change that occurs when an electron is acquired by naturopath and is called ______

A

Electron affinity

54
Q

Write an equation to Show an atom acquiring an electron and releasing energy

A

A+e –> A- + energy

55
Q

Whenever energy is released is assigned a ______ number

A

Negative

56
Q

If atoms are forced to gain an electron the energy involved would be assigned a ____number

A

Positive

57
Q

Which elements gain electrons most readily

A

Halogens

58
Q

In general as you move from left to right across Each period, Towards the halogens, elements tend to attract electrons more readily and have electron affinities becoming more ____

A

Negative

59
Q

The group of elements with the most negative electron affinities is group _______

A

17

60
Q

Moving down the periodic table within a group the electron affinity values become _______
Negative

A

More

61
Q

The elements n the periodic table has a _____tendency to add additional electronics

A

Lesser

62
Q

Hey cation is an ion with a _____ charge it is formed by the of one or more electrons

A

Positive; Loss

63
Q

Are cations bigger or smaller than the atoms from which they are formed?

A

Smaller

64
Q

An anion is an ion with a _____charge formed when an atom _____ electrons

A

Negative; gains

65
Q

Are anions larger or smaller than the Adam from which they are formed

A

Larger

66
Q

_____Electrons are available to be lost, gained, or shared in the formation of chemical compounds. They are generally found in the
_______ filled energy levels

A

Valence; Incompletely

67
Q

________Is a measure of the ability of an atom in a chemical compound to attract electrons

A

Electronegativity

68
Q

The element with the highest electronegativity is ____

A

Fluorine

69
Q

Describe the general area of the periodic table where elements with high electronegativities are located

A

In the lower left corner

70
Q

Where are the elements with lower Electronegativities Located

A

Lower left

71
Q

What are the possible islands formed by the iron atom

A

Fe+1, Fe2+, Fe3+

72
Q

What kind of ion do D block elements form?

A

2+ ions

chemistry reading guides (2 decks)

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