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×Chemistry 1 > The Periodic Law > Flashcards

The Periodic Law Flashcards

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1
Q

Dmitri Mendeleev

A

Russian chemist

developed and published the first periodic table of the elements

predicted the discovery of several new elements

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2
Q

Mendeleev’s periodic table

A

organized by increasing atomic mass

showed repeating (periodic) properties in columns

not perfect but highly accurate

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3
Q

Henry Moseley

A

English physicist

discovered that the elements in the periodic table fit into patterns better when they were arranged in increasing order according to the number of protons than by atomic mass

led to the definition of atomic number

rearranged the periodic table by atomic number

discovered the periodic law

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4
Q

periodic law

A

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

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5
Q

periodic table

A

an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column

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6
Q

groups

families

A

vertical columns on the periodic table

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7
Q

information given by groups

A

number of valance electrons in elements

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8
Q

quantum numbers given by groups

A

angular momentum quantum number

magnetic quantum number

spin quantum number

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9
Q

range of groups

A

1 to 18

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10
Q

periods

A

horizontal rows on the periodic table

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11
Q

information given by periods

A

number of energy levels in elements

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12
Q

quantum number given by periods

A

principal quantum number

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13
Q

range of periods

A

1 to 7

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14
Q

blocks

A

4 regions of the periodic table containing elements based on the electron configurations of elements

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15
Q

determination of blocks on periodic table

A

sublevel being filled in successive elements of that block

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16
Q

quantum number given by blocks

A

angular momentum quantum number

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17
Q

range of blocks

A

s

p

d

f

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18
Q

s-block

A

group 1 and group 2 on the periodic table

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19
Q

p-block

A

group 13 through group 18 on the periodic table

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20
Q

d-block

A

group 3 through group 12 on the periodic table

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21
Q

f-block

A

lanthanides series and actinide series on the periodic table

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22
Q

main group elements

A

s-block elements and p-block elements

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23
Q

general valence electron configuration of group 1

A

ns1

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24
Q

general valence electron configuration of group 2

A

ns2

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25
Q

general valence electron configuration of group 3

A

ns2(n-1)d1

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26
Q

general valence electron configuration of group 4

A

ns2(n-1)d2

27
Q

general valence electron configuration of group 5

A

ns2(n-1)d3

28
Q

general valence electron configuration of group 6

A

ns1(n-1)d5

29
Q

general valence electron configuration of group 7

A

ns2(n-1)d5

30
Q

general valence electron configuration of group 8

A

ns2(n-1)d6

31
Q

general valence electron configuration of group 9

A

ns2(n-1)d7

32
Q

general valence electron configuration of group 10

A

ns2(n-1)d8

33
Q

general valence electron configuration of group 11

A

ns1(n-1)d10

34
Q

general valence electron configuration of group 12

A

ns2(n-1)d10

35
Q

general valence electron configuration of group 13

A

ns2np1

36
Q

general valence electron configuration of group 14

A

ns2np2

37
Q

general valence electron configuration of group 15

A

ns2np3

38
Q

general valence electron configuration of group 16

A

ns2np4

39
Q

general valence electron configuration of group 17

A

ns2np5

40
Q

general valence electron configuration of group 18

A

ns2np6

41
Q

types of periodicity

A

atomic radii

ionic radii

ionization energy

electron affinity

electronegativity

shielding effect

chemical reactivity

42
Q

cation

A

positively charged ions

formed by the loss of all valence electrons in an element

made from atoms of metals

43
Q

oxidation

A

loss of electrons

44
Q

anions

A

negatively charged ions

formed by gaining enough electrons to obtain a noble gas configuration

made from atoms of nonmetals

45
Q

reduction

A

gain of electrons

46
Q

atomic radii

A

distance from the center of the nucleus of an atom to the border of the electron cloud

found by calculating half of the distance between the nuclei of identical atoms that are bonded together because there is no definite border of the electron cloud

47
Q

periodic trends of atomic radii

A

decreases from left to right

increases from top to bottom

48
Q

ionic radii

A

distance from the center of the nucleus of an ion to the border of an electron cloud

49
Q

ionic radii of cations (in comparison to an atom)

A

smaller than the atomic radius of a neutral atom due to loss of electrons

50
Q

ionic radii of anions (in comparison to an atom)

A

larger than atomic radius of a neutral atom due to gain of electrons

51
Q

periodic trends of ionic radii

A

decreases from left to right

increases from top to bottom

52
Q

ionization energy (IE)

A

amount of energy (in kJ/mol) needed to remove 1 electron from a neutral atom

53
Q

nth ionization energy (IEn)

A

energy (in kJ/mol) needed to remove an atom’s nth electron after the (n-1) electrons removed before it

54
Q

periodic trends of ionization energy

A

increases from left to right

decreases from top to bottom

55
Q

electron affinity (EA)

A

release of energy that occurs when an electron is acquired by a neutral atom

56
Q

periodic trends of electron affinity

A

increases from left to right

decreases from top to bottom

57
Q

reason for electron affinity of last group of each block to be equal to zero

A

final group of each block has filled all orbitals but new orbitals cannot be built for anions

58
Q

significance of a negative electron affinity value

A

represents amount of energy released

does not represent a negative measurement (not possible)

59
Q

electronegativity

A

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

based upon the arbitrarily assigned value of 4.0 to fluorine (most electronegative element)

60
Q

periodic trends of electronegativity

A

increases from left to right

decreases from top to bottom

61
Q

shielding effect

A

ability of inner electrons to pull on valence electrons

62
Q

periodic trends of shielding effect

A

constant from left to right

increases from top to bottom

63
Q

Jöns Jacob Berzelius

A

Swedish chemist

chose to use Latin to name the elements so that there was a unified name in a language that everybody understood

decided to give metals symbols with 2 letters

decided to give nonmetals symbols with 1 letter

64
Q

Stanislao Cannizzaro

A

Italian chemist

presented a convincing method for accurately measuring the relative masses of atoms

enabled chemists to agree on standard values for atomic mass and other properties of the elements

×Chemistry 1 (20 decks)

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