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Review Classes - Science > Chemistry [Introduction - Chemical Bonding] > Flashcards

Chemistry [Introduction - Chemical Bonding] Flashcards

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1
Q

Chemistry

A

Branch of science that deals with the characterization, composition, transformations, and the energies involved in the matter

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2
Q

Matter

A

anything that occupies space and has mass

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3
Q

Mass

A

the amount of matter that an object contains

expressed in terms of kilogram

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4
Q

Properties of Matter

A

Intensive or Extensive

Physical or Chemical

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5
Q

Intensive Property

A

depend on the quality of the matter

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6
Q

Extensive Property

A

depend on the quantity of the matter

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7
Q

Physical Property

A

directly observed or measured by an instrument

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8
Q

Chemical Property

A

requires another substance to react to

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9
Q

Example of Intensive (10)

A 
Volatility 
Viscosity
Malleability
Ductility
Alkalinity
Color
odor
Density
Boiling Point
Freezing Point
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10
Q

Example of Extensive (3)

A

Mass
Volume
Length

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11
Q

Examples of Physical Property (7)

A 
Temperature
Mass 
Color
Volatility
Viscosity
Malleability
Ductility
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12
Q

Examples of Chemical Property (3)

A

Combustibility
Acidity
Alkalinity

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13
Q

Classical Phases of Matter

A

Solid
Liquid
Gas

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14
Q

Solid

A

strong attractive force between particles of matter

definite volume and shape

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15
Q

Two types of Solid

A

Amorphous - without definite structure

Crystallize - with definite structure

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16
Q

Liquid

A

weak attractive force
definite volume and indefinite shape
flows in one direction

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17
Q

Gas

A

attractive force is almost inexistant
indefinite volume and shape
flows in random directions

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18
Q

Physical Change

A

Transformation from one phase to another

Molecules are not affected

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19
Q

Chemical Change

A

involves the formation of a new substance

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20
Q

Evidences of Chemical Change

A

Change in color of solution
Formation of a precipitate
Evolution of gas
Absorption or Evolution of heat

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21
Q

Classification of Matter

A

Matter : Pure Substance and Mixture

Pure substance: Elements and Compounds
Elements: nonmetals, metals, metalloids
Compound: ionic and covalent

Mixture: Homogeneous and Heterogeneous
Homogeneous: Solutions
Heterogeneous: Colloids and Suspensions

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22
Q

Pure Substance

A

Uniform Composition with distinct physical ad chemical properties

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23
Q

Elements

A

simplest substance

made up of only one type of atom

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24
Q

Compounds

A

made up of two or more different atoms combined in different proportions

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25
Q

Ionic Compounds

A

metal + nonmetal

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26
Q

Covalent Compounds

A

nonmetal + nonmetal

sharing of electrons

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27
Q

Mixture

A

physical combination of two or more substances

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28
Q

Homogeneous mixture

A

uniform in composition and properties
a single phase is observable
size of particles are the smallest of all Mixtures

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29
Q

Components

A

used to identify substances in a mixture

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30
Q

Solvent

A

used to dissolve the solute
usually present in greater amount
determines the state of the matter

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31
Q

Solute

A

being dissolved in the solvent

usually present in small amount

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32
Q

Types of Solutions based on Concentration of Solute

A

Diluted

Concentrated

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33
Q

Types of Solutions Based on the Capacity to dissolve a Solute

A

Unsaturated
Saturated
Supersaturated

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34
Q

Diluted

A

low amount of solute

35
Q

Concentrated

A

large amount of solute

36
Q

Unsaturated

A

lesser amount of solute than what is required to make it saturated

37
Q

Saturated

A

very concentrated solution

any added solute will no longer be dissolved

38
Q

Supersaturated

A

solute greater than that of a saturated solution

39
Q

Solubility

A

ability of a solute to dissolve in a solvent

40
Q

Heterogenous Mixture

A

components separate into distince phases

41
Q

Suspension

A

Suspended particles tend to settle ad separate from the medium

42
Q

Colloid

A

particles remain at afloat and never settle but can still be seen

43
Q

Properties of Colloid

A

Tyndall Effect
Brownian Movement
Adsorption
Electrical Property

44
Q

Tyndall Effect

A

scattering of light

45
Q

Brownian Movement

A

random movement of particles

46
Q

Adsorption

A

adhesion of atoms, ions, or molecules to a surface

47
Q

Separation Techniques

A 
Filtration
Distillation
Crystallization
Fractional Distillation
Chromatography
48
Q

Filtration

A

Insoluble solid

has Precipitate/Residue and Filtrate

49
Q

Distillation

A

Solid in a liquid

obtains liquid through steam

50
Q

Crystallization

A

Solid in a liquid

obtains the solid

51
Q

Fractional distillation

A

two miscible liquid

52
Q

Chromatography

A

mixture of small amount of solids

53
Q

Postulates of Dalton’s Atomic theory

A
  1. Elements are composed of indivisible particles called atoms
  2. Atoms of the same (different) element possess identical (different) properties.
  3. Atoms are neither created, destroyed nor changed
  4. Atoms combine in fixed ratios of whole numbers forming molecules
54
Q

Electron, e-

A

carries negative electric charge and found outside the nucleus of an atom

55
Q

Proton, p+

A

carries positive electric charge ad found in the nucleus

56
Q

Neutron, n^0

A

electrically neutral and found in the nuclues

57
Q

Atomic Mass, A

A

number of protons + number of neutron

58
Q

Atomic Number, Z

A

number of protons (in neutral atoms, this is equal to the number of electrons)

59
Q

Ions

A

formed when atoms lose or gain electrons

60
Q

Cations

A

positively charged ions, formed when an atom loses one or more electrons

61
Q

Antions

A

negatively charged ions, forced then an atoms gain one or more electrons

62
Q

Isotoped

A

atoms of the same elements with different number of neutrons and different atomic mass

63
Q

Principle Quantum Number, n

A

denotes the shell or the main energy level in which the electron is found

64
Q

Azimuthal Quantum number, l

A

denotes the subshell and determines the shape of the orbital

65
Q

Magnetic Quantum number, ml

A

identifies the orbital where the electron is situated

66
Q

Spin Quantum number, ms

A

determines the direction of the spin of the electron

67
Q

Electron Configuration

A

number, distribution, or arrangement of electrons

68
Q

Aufbau Principle

A

states that electrons fill up the lowest energy level first

69
Q

Hund’s Rule of Maximum Multiplicity

A

electrons occupy separate orbitals in the same subshell with parallel spins

70
Q

Pauli’s Exclusion Principle

A

no two electrons will have the same set of quantum numbers

71
Q

Group/Family

A 
each vertical column in the periodic table 
Group 1 - Alkali Metals
Group 2 - Alkaline Metals
Group 13 - Boron Group
Group 14 - Carbon Group
Group 15 - Nitrogen Group
Group 16 - Oxygen Group
Group 17 - Halogens
Group 18 - Noble or Inert Gases
72
Q

Period/Series

A

each horizontal row

the period number determines the ordinal value of the outermost shell

73
Q

Classification of Elements

A

Metals
Nonmentals
Metalloids

74
Q

Periodic Law

A

atoms of different elements are arranged in increasing atomic number, periodic properties are observed

75
Q

Atomic Radius

A

size of an atom

distance from the nucleus to the outermost electron

76
Q

Electronegativity

A

Tendency of a bonded atom to attract electrons in a covalent bond

77
Q

Ionization Energy

A

the minimum energy required to remove an electron from the outermost shell of a gaseous atom

78
Q

Electron Affinity

A

the energy released when a gaseous atoms gains an extra electron

79
Q

Metallicity

A

describes properties such as conductivity, ductility, malleability

80
Q

Chemical Bonds

A

Ionic Bounds

Covalent : Polar and Nonpolar

81
Q

Ionic Bounds

A

Losing (metal) and gaining (non-metal) of electrons

82
Q

Covalent Bonds

A

sharing of electrons

83
Q

Polar Covalent

A

partially positive and a slightly negative region between atoms
unequal sharing of electrons (one is more electronegative than the other)

84
Q

Non-polar Covalent

A

electrons are shared equally and present in homonuclear diatomic molecules

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