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Grade 9 Lessons : 2nd Quarter > SCIENCE 9: 2nd Quarter > Flashcards

SCIENCE 9: 2nd Quarter Flashcards

1
Q

Anything that has mass

A

Matter

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2
Q

Smallest unit of matter

A

Atom

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3
Q

A.P.E

A

Atomic # found on top of the element’s symbol is equivalent to the protons and electrons.

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4
Q

Greek Philosopher

A

Democritus

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5
Q

He named the smallest piece of matter “atomos” means not to be cut.

A

Democritus

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6
Q

He said that it is all small, hard particles that are made of same material but different shapes and sizes.

A

Democritus

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7
Q

He said that all elements are composed of atoms.

A

John Dalton

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8
Q

Atoms of the same elements are alike, atoms of different elements are different.

A

John Dalton

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9
Q

Introduced electron

A

Joseph John Thomson

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10
Q

His experiment is the “Plum Pudding”.

A

Joseph John Thomson

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11
Q

He said positive atoms (protons) are inside at the nucleus, and the negative charged are outside the nucleus scattered.

A

Ernest Rutherford

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12
Q

Proposed an improvement, each electron are in a specific energy level, it moved in definite orbits around the nucleus.

A

Niels Bohr

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13
Q

Modified Niels Bohr atomic theory to include elliptical orbits.

A

Arnold Sommerfeld

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14
Q

Father of quantum mechanics

A

Erwin Schrondinger

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15
Q

Today’s atomic model is based on the principles of wave mechanics. Electrons whirl, electrons don’t move around atom in definite path, it also does not move in random patterns.

A

Erwin Schrondinger

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16
Q

Discovered protons

A

Eugene Goldstein

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17
Q

Study of waves

A

Quantum Mechanics

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18
Q

Discovered Neutrons

A

James Chadwick

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19
Q

Smallest particle of an element

A

Atoms

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20
Q

Smallest amount of substance that can take part in any chemical reaction

A

Atom

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21
Q

He said that atoms are made of positively charged particle with negatively charge electrons

A

Joseph, John Thomson

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22
Q

When sodium and chlorine bond they make the ___ sodium chloride

A

Compound

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23
Q

When two or more elements bond they make a??

A

Compound

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24
Q

They have different properties than the elements that make them up

A

Compound

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25
Q

Sodium+ chlorine=

A

Sodium chloride= table salt

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26
Q

Compounds in ___ retain their individual properties

A

Mixtures

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27
Q

It is a substance composed of two or more elements chemically bonded together.

A

Compound

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28
Q

It is a combination of different substances that are not chemically bonded

A

Mixture

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29
Q

It can be separated by physical means

A

Mixture

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30
Q

Can only be separated by chemical means

A

Compounds

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31
Q

Are pure substances

A

Elements

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32
Q

Group, 14 to 17

A

Nonmetals

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33
Q

Nonmetals

A

Groups, 14 to 17

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34
Q

Metals

A

Group one to 13

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35
Q

Group 1to 13

A

Metals

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36
Q

Noble gas

A

Group 18

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37
Q

The group number will give you an idea of the

A

Number of valence electron

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38
Q

The __ will give you an idea of the number of valence electrons

A

Atomic number

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39
Q

S Block

A

Group one, and two

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40
Q

P block

A

Group, 13 to 18

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41
Q

Metals have __ valence electrons

A

Low

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42
Q

Non-metals have __ valence electron

A

High

43
Q

All noble gas has __ valence electrons

A

Eight

44
Q

What do you notice in the number of valence electrons of metals, nonmetals and noble gases?

A

Metals have lesser valence electrons than nonmetals. All noble gases have eight valence electron.

45
Q

Electrons in the outermost energy level

A

Valence electron

46
Q

Electrons that are transferred or shared when atoms bond together

A

Valence electron

47
Q

Energy needed to remove outermost valance electrons

A

Ionization

48
Q

Tendency of an atom to attract valence electrons

A

Electronegativity

49
Q

What do you notice with the number of valence electrons, electronegativity values, and ionization energies of the element?

A

As the number of valence electron increases, electronegativity and ionization also increases

50
Q

What kind of element has the greatest tendency to attract electrons why?

A

Nonmetals have the greatest tendency to attract electrons because they have high electronegativity

51
Q

What kind of elementary was high energy to remove its valence electrons why?

A

Nonmetals have high energy requirements to pull its valence electron

52
Q

It tells you that elements gain or loose or share electrons to achieve the electronic configuration of the nearest noble gas

A

The octet rule

53
Q

After chemical bonding elements become __ with the nearest noble gas

A

Isoelectronic

54
Q

Same electrons, even though different atomic numbers

A

Isoelectronic

55
Q

Our areas within shells where the electrons are located

A

Orbitals

56
Q

We know that electron is somewhere in the orbital, but we can’t know exactly where it is or how fast it is moving

A

Heinsberg’s uncertainty principle

57
Q

Is the arrangement of electrons around the nucleus based on their energy level?

A

Electronic configuration

58
Q

Electrons are added one at a time to the lowest energy level first

A

Aufbau principle

59
Q

Two elections in same orbital have different spins

A

Pauli exclusion principle

60
Q

When electrons are filling orbitals of the same energy, they prefer to enter empty, orbitals first. These electrons all have the same spin.

A

Hund’s Rule

61
Q

The transfer of electrons

A

Ionic band

62
Q

The form between metals and nonmetals

A

Ionic bond

63
Q

It dissolves easily in water

A

Ionic compounds

64
Q

It easily conduct electricity

A

Ionic compound

65
Q

It tends to form crystals with high melting temperature

A

Ionic compound

66
Q

Bonding by sharing

A

Covalent bonding

67
Q

Two types of covalent bond

A

Polar and nonpolar

68
Q

Non-identical atoms with electronegativity higher than 0.4 and lower than 1.9

A

Polar

69
Q

Two identical, non-metallic atoms, such as nitrogen, oxygen, fluorine, and diatomic particles

A

Nonpolar

70
Q

Diatomic elements

A

Have no fear of ice cold bromine

71
Q

Compounds that are primarily composed of carbon atoms

A

Organic compounds

72
Q

Are naturally produced by living organisms, but can also be produced artificially

A

Organic compounds

73
Q

Carbon atoms have __ valence electrons

A

4

74
Q

To identify organic compounds

A

Physical properties, boiling point density, color, smell, and stability

75
Q

Organic compounds examples

A

Gasoline kerosene, LPG, ethanol, acetone and acetic acid

76
Q

Low electronegativity

A

Metals

77
Q

High electronegativity

A

Nonmetals

78
Q

Metals have less than __ valence electrins

A

4

79
Q

Nonmetals have more than __ valence electrons

A

4

80
Q

Symbol with dot around

A

Lewis symbol

81
Q

Ionization group trend

A

As you go down a column ionization energy decreases

82
Q

Ionization period trend

A

As you go left or right, it increases

83
Q

Electronegativity periodic trend

A

As you go, left or right electronegativity increases

84
Q

Electronegativity group trend

A

As you go down a column electronegativity decreases

85
Q

Atomic radius group trend

A

As you go down a column atomic radius increases

86
Q

Atomic radius, periodic trend

A

As you go left or right atomic radius decreases

87
Q

Unsaturated

A

Alkene and alkyne

88
Q

Saturated

A

Alkane

89
Q

Single bond

A

Alkane

90
Q

Double bond

A

Alkene

91
Q

Triple bond

A

Alkyne

92
Q

Composed of hydrogen and carbon

A

Hydrocarbon

93
Q

4 carbon to be stablr

A

Hydrocarbon

94
Q

1 carbon

A

Meth

95
Q

2 carbon

A

Eth

96
Q

3 carbon

A

Prop

97
Q

4 carbon

A

But

98
Q

5 carbon

A

Pent

99
Q

6 carbon

A

Hex

100
Q

7 carbon

A

Hept

101
Q

8 carbon

A

Oct

102
Q

9 carbon

A

Non

103
Q

10 carbon

A

Dec

Grade 9 Lessons : 2nd Quarter (5 decks)

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