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Chemistry🌿 > Final 9 Teoria > Flashcards

Final 9 Teoria Flashcards

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1
Q

Science that studies the properties of matter and its changes

A

Chemistry

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2
Q

Anything that takes up space and has mass

A

Matter

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3
Q

Capacity to do work

A

Energy

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4
Q

Physical combination of two or more substances, in which the distinct identities are retained

A

Mixture

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5
Q

Atoms of the same element with different mass but the same atomic number

A

Isotope

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6
Q

Information that indicates the location of the electrons in the atom

A

Quantum numbers

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7
Q

Notation that shows how the electrons are distributed among the atomic orbitals and energy levels

A

Electronic configuration

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8
Q

Principle that establishes that each new electron added to an atom, will enter in the available orbital with less energy

A

Aufbau’s Principle

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9
Q

Rule that says that the electrons are going to enter each orbital with a parallel spin until all orbitals are complete

A

Hund’s Rule

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10
Q

Rule that claims that electrons in the same atom cannot have the same four quantum numbers, they must have opposite spins

A

Paulli’s Rule

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11
Q

Attraction forces that hold atoms together

A

Chemical bond

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12
Q

Establishes that atoms can become stable by having eight electrons in the outer energy level

A

Octet rule

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13
Q

Type of bond that is made between metals and non-metals where one of the atoms loses electrons and the other atom gains them.

A

Ionic bond

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14
Q

Electrostatic attraction in which a hydrogen atom forms a bridge between two electronegative elements

A

Hydrogen bond

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15
Q

One half of the distance between the nuclei of identical atoms bonded together

A

Atomic radius

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16
Q

Energy required to remove one electron from a neutral atom of an element

A

Ionization energy

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17
Q

A single kind of matter with a specific composition and properties

A

Pure substance

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18
Q

Matter is the same, the original matter can be recovered, and the particles of the substance are rearranged

A

Physical change

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19
Q

Matter is different, the old matter is no longer present and cannot be reverted, and particles are broken apart forming a new substance

A

Chemical change

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20
Q

What are the subatomic particles?

A

The particles that make up an atom:

Electron (-)

Proton (+)

Neutron (+-)

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21
Q

Notations used to show now the orbitals of a sup-shell are occupied by electrons.

A

Diagram of orbitals

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22
Q

Is defined as the change in energy of a neutral atom when an electron is added to the atom to form a negative ion.

A

Electron affinity

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23
Q

Attraction force between the nuclei of non-metals and the pair of electrons that is shared between them.

A

Covalent bond

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24
Q

Examples of heterogeneous mixtures

A

Water and oil

Sandwich

Salad

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25
Q

Examples of homogeneous mixtures

A

Sea water

Tequila

Sand and water

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26
Q

Mention 3 separation methods

A

Magnetism

Chromatography

Distillation

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27
Q

Magnetism

A

Involves using a magnet to attract another magnetic object away from the substance it is in

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28
Q

Chromatography

A

The process of separating colored chemicals

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29
Q

Distillation

A

The substances separates with heat

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30
Q

States of matter

A

Solid

Liquid

Gas

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31
Q

Solid

A

Retains a fixed volume and shape

Little free space between particles

Rigid particles cannot move

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32
Q

Liquid

A

Assumes the shape of part of the container which it occupies.

Not easily compressible.

Flows easily.

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33
Q

Gas

A

Assumes the shape and volume of its container.

Compressible

Flows easily

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34
Q

Timeline representing the evolution of the atom

A

Dalton

Thomson

Rutherford

Chadwick

Bohr

Sommerfeld

Schrödinger Heisenberg

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35
Q

Families’ names of the periodic table

A

Alkali metals

Alkaline earthmetals

Transition metals

Earth

Carbon family

Nitrogen familiy

Oxygen family

Halogens

Inert Noble Gases

(LOS DE ABAJO DE LA PERIODIC TABLE)

Lathanide series
Actinide series

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36
Q

Characteristics of the metals

A

Good conductors

Ductile

Crystal structure

High densities

Most of them solid

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37
Q

Characteristics non-metals

A

Poor conductors

Brittle

Low densities

Low melting points

Dull appearance

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38
Q

Characteristics of the metalloids

A

Semi-conductors

Solid and may have luster

Similar properties to metals and non-metals

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39
Q

H

A

Hydrogen

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40
Q

Li

A

Lithium

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41
Q

Na

A

Sodium

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42
Q

K

A

Potassium

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43
Q

Rb

A

Rubidium

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44
Q

Be

A

Beryllium

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45
Q

Mg

A

Magnesium

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46
Q

Ca

A

Calcium

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47
Q

Sr

A

Strontium

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48
Q

Ba

A

Barrium

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49
Q

Radium

A

Ra

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50
Q

Boron

A

B

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51
Q

Aluminium

A

Al

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52
Q

Gallium

A

Ga

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53
Q

Carbon

A

C

54
Q

Silicon

A

Si

55
Q

Fluorine

A

F

56
Q

Chlorine

A

Cl

57
Q

Bromine

A

Br

58
Q

Iodine

A

I

59
Q

N

A

Nitrogen

60
Q

P

A

Phosphorus

61
Q

As

A

Arsenic

62
Q

Sb

A

Antimony

63
Q

Bi

A

Bismuth

64
Q

O

A

Oxygen

65
Q

S

A

Sulfur

66
Q

Rn

A

Radon

67
Q

Co

A

Cobalt

68
Q

Ni

A

Nickel

69
Q

Astatine

A

At

70
Q

Helium

A

He

71
Q

Neon

A

Ne

72
Q

Argon

A

Ar

73
Q

Krypton

A

Kr

74
Q

Xenon

A

Xe

75
Q

Mercury

A

Hg

76
Q

Gold

A

Au

77
Q

Platinum

A

Pt

78
Q

Silver

A

Ag

79
Q

Cu

A

Copper

80
Q

Zn

A

Zinc

81
Q

Pd

A

Palladium

82
Q

Sn

A

Tin

83
Q

Cd

A

Cadmium

84
Q

Ti

A

Titanium

85
Q

W

A

Tungsten

86
Q

Cr

A

Chromium

87
Q

Mn

A

Manganese

88
Q

Fe

A

Iron

89
Q

Pb

A

Lead

90
Q

Kg -> g

A

*1000

91
Q

G -> kg

A

/1000

92
Q

Ml -> L

A

/1000

93
Q

L -> ml

A

*1000

94
Q

KG=

A

L

95
Q

G=

A

ML

96
Q

(S)

A

Solid

97
Q

(g)

A

Gas

98
Q

(l)

A

Liquid

99
Q

(aq)

A

Aqueous

100
Q

(triangle)

A

Heat

101
Q

(Arrow looking up)

A

Escape of gas

102
Q

Arrow looking down

A

Precipitation

103
Q

(Thunder)

A

Electric current

104
Q

Aufbau’s Principle

A 
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p
105
Q

VALUES “s,p,d,f” for electron configuration

A

S= 2

P= 6

D= 10

F= 14

106
Q

Values “s,p,d,f” for the quantum number “l”

A

S= 0

P= 1

D= 2

F= 3

107
Q

Percent by mass formula

A

Mass of solute/mass of solution *100

108
Q

Percent by volume formula

A

Volume of solute/volume of solution *100

109
Q

Molarity formula

A

Moles of solute/liter of solution

110
Q

Molality formula

A

Moles of solute/kilogram of solvent

111
Q

Mole fraction formula

A

Moles of solute/ moles of solute + moles of solvent

112
Q

Dilution formula

A

C1 (V1) = C2 (V2)

113
Q

Units for % volume

A

Solute= ml

Solution= ml

% volume= %

114
Q

Units for % mass

A

Solute= g

Solution= g

% mass= %

115
Q

Units for molarity

A

Solute= moles

Solution= liters

Molarity= M

116
Q

Units for molality

A

Solute= moles

Solvent= kg

Molality= m

117
Q

Units for mole fraction

A

Solute= moles

Solvent= moles

Mole fraction= no units

118
Q

Units for dilution

A

Volume= ml

Concentration= M

119
Q

Atomic radius/ metallic character

A

-

+ -

120
Q

Ionization energy/ electron affinity/ electronegativity

A

+

  • +
121
Q

Synthesis

A

A + B > AB

122
Q

Decomposition

A

AB > A + B

123
Q

Single replacement

A

AB + C > AC + B

124
Q

Double replacement

A

AB + CD > AD + BC

125
Q

Combustion

A

> CO2 + H2O

126
Q

Neutralization

A

OH

127
Q

Cation

A

Positive value

128
Q

Anion

A

Negative value

129
Q

Si el valor es menor que 0.4

A

Covalent non polar

130
Q

Si el valor es mayor es mayor que 0.4 pero menor que 1.7

A

Covalent polar

131
Q

Si el valor es mayor que 1.75

A

Ionic

Chemistry🌿 (3 decks)

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