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INORGANIC AND ORGANIC CHEMISTRY > ATOMS AND PERIODIC TABLE > Flashcards

ATOMS AND PERIODIC TABLE Flashcards

1
Q

a positive charge particles

A

Proton

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2
Q

no charge associated with it

A

Neutron

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3
Q

negative electrical charge, smallest in terms of mass

A

Electrons

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4
Q

found at the center of an atom

A

all protons and all neutrons

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5
Q

the outer region of an atom contains

A

all the electrons

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6
Q

a subatomic particle found in the nucleus of an atom

A

Nucleon

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7
Q

placed as a superscript; above

A

Mass number

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8
Q

placed as a subscript; below

A

Atomic number

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9
Q

A= number of protons + number of neutrons

A

Mass number

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10
Q

z = number of protons = number electrons

A

Atomic number

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11
Q

determined by the numbers and arrangement of electrons about the nucleus

A

Chemical Properties of an atom

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12
Q

pure substance in which all atoms present have the same atomic number

A

Element

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13
Q

atoms of an element that have the same of protons and the same number of electrons but different numbers of neutrons

A

Isotopes

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14
Q

calculated average mass for the isotopes of an element, expressed on a scale where 12/6 C serves as the reference point

A

Atomic Mass

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15
Q

states that when elements are arranged in increasing atomic number, elements with similar chemical properties occur in periodic (regularly recurring) intervals

A

Periodic Law

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16
Q

A tabular arrangement of the elements in order of increasing atomic number such that elements having similar chemical properties are positioned in vertical columns

A

Periodic Table

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17
Q

a horizontal row

A

Period

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18
Q

a vertical column

A

Group

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19
Q

An element that has the characteristic properties of luster, thermal conductivity, electrical conductivity, and malleability

A

Metal

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20
Q

an element characterized by the absence of properties of luster, thermal conductivity, electrical conductivity and malleability

A

Nonmetal

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21
Q

the majority of the elements are

A

Metal

  • Approximately 93 elements are metals, depending on how the artificially synthesized elements are classified. Only about 18 of the elements are classified as nonmetals.
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22
Q

restricted to specific regions within the extranuclear portion of the atom

A

Electrons

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23
Q

limited to certain values, and a specific behavior is associated with each allowed energy value

A

Electron Energies

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24
Q

the space in which electrons move rapidly about is divided into subspaces called (3)

A

Shells
Subshells
Orbitals

25
Q

he developed theory about atom which is known as dalton’s atomic theory

A

John Dalton (1803) in my notes (1802)

26
Q

a region of space about a nucleus that contains electrons that gave approximate the same energy and that spend most of their approximately the same distance from the nucleus

A

Electron Shell

27
Q

Electron shells are numbered by

A

1, 2 ,3 and so on, outwards from the nucleus

28
Q

a region of space within an electron shell that contains electrons that have the same energy

A

Electron subshell

29
Q

the number of subshell within a shell is the same as the

A

shell number

30
Q

differ in size, and each type is designated using the letters s,p,d and f

A

Subshells

31
Q

subshell with 2 electrons

A

s subshell

32
Q

subshells with 6 electrons

A

p subshell

33
Q

subshell with 10 electrons

A

d subshell

34
Q

subshell with 14 electrons

A

f subshell

35
Q

used in identifying subshells

A

Both number and a letter

36
Q

gives the shell within which the subshell is located

A

Number

37
Q

gives the type of subshell

A

Letter

38
Q

a region of space within an electron subshell where an electron with a specific energy

A

Electron Orbital

39
Q

can accommodate maximum of 2 electrons

A

Electron Orbitals

40
Q

( 2 electrons) contains one orbital

A

s subshell

41
Q

(6 electrons) contains three orbitals

A

p subshell

42
Q

(10 electrons) contains five orbitals

A

d subshell

43
Q

(14 orbitals) contains seven orbitals

A

f subshell

44
Q

orbitals: spherical in shape

A

S orbital

45
Q

orbitals: have shaped similar to to the figure 8

A

p orbitals

46
Q

orbitals: a clover shape

A

d orbital

47
Q

orbitals: no definite shape

A

f orbital

48
Q

Electron subshells are filled in order of

A

increasing energy

49
Q

however, energies of subshells in different shelf

A

overlap

50
Q

the 4s subshell has lower energy that the

A

3d subshell

51
Q

dictates the manner in which electrons are filled in the atomic orbitals of an atom in its ground state.

A

Aufbau Principle or Aufbau Rule

52
Q

a statement of how many electrons an atom has in each of its electron subshells

A

Electron Configuration

53
Q

superscipt following each subshell designation indicated the

A

number of electrons in that subshell

54
Q

written in symbols; using number-letter combination

A

Electron Configuration

55
Q

groups (columns) of elements have similar chemical properties because similarities in their what

A

electron configuration

56
Q

how many orbitals are there in s subshell

A

1 orbital

57
Q

how many orbitals are there in p subshell

A

3 orbitals

58
Q

how many orbitals are there in d subshell

A

5 orbitals

59
Q

how many orbitals are there in f subshell

A

7 orbitals

INORGANIC AND ORGANIC CHEMISTRY (7 decks)

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