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CIDEB Chemistry 1 > Stage 3 > Flashcards

Stage 3 Flashcards

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0
Q

Neutron

A

Neutral subatomic particle int he nucleus of an atom.

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1
Q

Proton

A

Positively charged subatomic particle inside the nucleus of an atom.

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2
Q

Electron

A

Negatively charged subatomic particle that is floating around the nucleus in the electron cloud. It is the smallest type of subatomic particles and they are part of chemical reactions.

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3
Q

Atomic number

A

Number of protons (or electrons Ina neutral atom) in an atom.

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4
Q

Atomic mass

A

The average of the weights of all the natural occurring isotopes of an element.

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5
Q

Mass number

A

Sum of the protons and neutrons in an atom’s nucleus.

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6
Q

Electron configuration

A

Shows the arrangements of e- in an atom

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7
Q

Atomic theories

A

Democritus, dalton, Thomson, Rutherford, Bohr, Schrödinger.

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8
Q

Atoms

A

Basic unit of all matter that contains the properties of an element.

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9
Q

Radioactivity

A

Release of energy by the atoms. Propriety.

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10
Q

Types of radiation

A

Alpha, beta and gamma

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11
Q

Example of radioactive elements

A

Plutonium (239), cobalt (60) and strontium (90)

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12
Q

S block

A

Groups 1A & 2A ink using including hydrogen and helium.

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13
Q

P block

A

3A - 8A! Excluding helium.

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14
Q

D block

A

Transition metals

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15
Q

F block

A

Inner transition metals (lanthanides and actinides)

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16
Q

Groups or families

A

Columns

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17
Q

Periods

A

Rows

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18
Q

Ionization energy periodic trend

A

It increases as you go up in a family and right in a period.

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19
Q

Electronegativity periodic trend

A

It increases as you go up in a family and right in a period.

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20
Q

Element with the highest electronegativity

A

Fluorine

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21
Q

Elements that have a high ionization energy but no electronegativity

A

Noble gases

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22
Q

Periodic trend in atom in radius

A

It increases as you go down in a family and left in a period.

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23
Q

Greek philosophers thought that matter …

A

Was made from four elects (air, water, fire and earth) and could be endlessly divided.

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24
Q

Democritus

A

Matter is made from tiny individual particle that cannot be created destroyer nor divided.

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25
Q

Main contributions of John Dalton

A

He was the first one to sustain the fact that everything is made out of worms, he said that atoms of difference elements had different weights, that everything was made up of atoms and that toms were the smallest indivisible particle.

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26
Q

Principle of Dalton’s model

A
  1. Everything is made out of atoms. They are indivisible and indestructible.
  2. Atoms cannot be created nor destroyed.
  3. atoms of the same element have the same size, chemical properties and mass. They are different from atoms of other elements.
  4. Atoms of different elements combine to form compounds.
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27
Q

Dalton was wrong because …

A

He didn’t include the subatomic particles and because isotopes of the same element have different masses.

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28
Q

Laws used by dalton

A

Law of conservation of mass
Law of constant competition/ definite properties
Law of multiple proportions

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29
Q

Law of conservation of mass

A

Mass cannot be created nor destroyed, only transformed

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30
Q

Thomson’s model

A

Plum pudding model

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31
Q

Main contribution of Thomson

A

Addition of electrons to the atomic model.

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32
Q

Thomson’s experiment

A

Used a cathode-ray tube (electron gun) to create negative ways made from negative particles that were deflected by a positive wave between magnets.

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33
Q

Description of Thomson’s model

A

Negative charged particles (plums) swimming in a sea of positive charge (pudding)

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34
Q

Thomson was wrong because …

A

He didn’t mention the nucleus.

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35
Q

Rutherford’s main contribution

A

The inclusion of the positively charged nucleus by a bunch of negatively charges particles.

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36
Q

Rutherford’s experiment

A

Gold foil experiment. He fire we alpha particles at a foil expecting them to be rejected.

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37
Q

Description of Rutherford’s model

A

Positively charge nucleus in which most of the atom’s mass is located surrounded by circulating electrons.

38
Q

Rutherford’s model

A

Nuclear atom

39
Q

Rutherford was wrong because …

A

His model did not explain the electron arrangement and in this model the electrons would eventually collide with the nucleus.

40
Q

Bohr’s model

A

Solar system model

41
Q

Bohr’s main contribution

A

Implementation of electron orbits (shells [energy levels] and levels)

42
Q

Bohr was wrong because …

A

Its model could not be used for atoms more complicated than hydrogen.

43
Q

Photon

A

Massless particle that contains quantum energy and that is real eased when an electron passes from its exited state into its ground state.

44
Q

Ground states

A

The lowest allowable energy state

45
Q

Exited state

A

When an atom gains energy

46
Q

When does scent so observed that elements have of visible light

A

When heated by flame

47
Q

Schrödinger’s model

A

Quantum mechanical model

48
Q

Main contribution Schrödinger

A

Inclusion of electron orbitals.

49
Q

Characteristic of the quantum mechanical model

A

It can help us calculate the probability of finding an electron in a particular volume of space close to the nucleus.

50
Q

Atomic orbital

A

Region around a nucleus in which it is described an elctron’s probable location in the electron clouds.

51
Q

Heisenberg uncertainty principle

A

It is impossible to know the location and velocity of a particle at the same time. So you can only know the probability of an electron to occupy a certain region around the nucleus.

52
Q

Proton charge

A

+1

53
Q

Proton symbol

A

P+

54
Q

Proton discover

A

Rutherford in 1919 with the gold foil experiment.

55
Q

Neutron charge

A

0

56
Q

Neutron symbol

A

n0

57
Q

Neutron discovery

A

Chadwick in 1932 while examinating penetrating radiation

58
Q

Electron change

A

-1

59
Q

Electron symbol

A

e-

60
Q

Electron discovery

A

Thomson in 1897 wile testing and measuring the cathode Rays.

61
Q

Isotope

A

Atoms with the same number of protons but different number of neutrons.

62
Q

Isotopic notation

A

A
X
Z

63
Q

A

A

Mass number (p+ + n0)

64
Q

Z

A

Atomic number

65
Q

of p+ (atomic number)

A

Z

66
Q

X

A

Symbol of the element

67
Q

Energy level

A

Possible orbits in which the elctrons may be found

68
Q

Sublevels

A

Divisions of the energy levels into s, p, d, f,

69
Q

Orbitals

A

Spaces that have a high probability of continuing an electron.

70
Q

Sublevels s

A

1 orbital 2e

71
Q

Sublevels p

A

Orbital 3 6 e

72
Q

D subshell

A

5 orbitals and 10 e

73
Q

F sushell

A

7 orbitals and 14 e-

74
Q

Electron configuration

A

the arrangement of electrons in an atom.

75
Q

Orbital diagram

A

Diagram that shows how the orbit in a subshell are occupied by electrons.

76
Q

Abbreviated notation

A

Noble has notation

77
Q

Diagonal rule

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

78
Q

Quantum number

A

Their combination tells the location of an specific electron

79
Q

Type of quantum numbers

A
  1. N, l, m, x
80
Q

N

A

Principal level

81
Q

L

A

Angular sublevels

82
Q

M

A

Magnetism orbitals

83
Q

S

A

Spin 1/2 or -1/2

84
Q

Gold rule

A

No two e- will have the same 4 quantum numbers.

85
Q

Aufbau principle

A

Each electron occupies the lowest energy orbitals available.

86
Q

Hund’s rule

A

Single electrons with the same spin must occupy equal orbital before additional electrons with apposite spins occupy.

87
Q

Name of each family

A 
Alkali metals 
Alkaline earth metals
Boron family
Carbon family
Nitrogen family
Oxygen party or chalcogens
Halogens
Noble gases.
88
Q

Oxidation number for each family

A

+1, +2, +3, +4 or -4, -3, -2, -1.

89
Q

Octet rule

A

Atoms will gain, lose or share electrons to acquire a full set of eighth valence electrons.

90
Q

Electronegativity

A

Ability of an element to attract electrons in a chemical bond.

91
Q

Atomic radius

A

Distance between the valence electrons and the nucleus.

92
Q

Ionization energy

A

Energy require to remove an electron from an atom.

93
Q

Valence electrons

A

They are the electrons in the outermost energy level, hey determine the charactestics of a compound and they also made a shame of them selves

CIDEB Chemistry 1 (2 decks)

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