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

Chemistry [Introduction - Chemical Bonding] Flashcards

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
Ionic Compounds
metal + nonmetal
26
Covalent Compounds
nonmetal + nonmetal | sharing of electrons
27
Mixture
physical combination of two or more substances
28
Homogeneous mixture
uniform in composition and properties a single phase is observable size of particles are the smallest of all Mixtures
29
Components
used to identify substances in a mixture
30
Solvent
used to dissolve the solute usually present in greater amount determines the state of the matter
31
Solute
being dissolved in the solvent | usually present in small amount
32
Types of Solutions based on Concentration of Solute
Diluted | Concentrated
33
Types of Solutions Based on the Capacity to dissolve a Solute
Unsaturated Saturated Supersaturated
34
Diluted
low amount of solute
35
Concentrated
large amount of solute
36
Unsaturated
lesser amount of solute than what is required to make it saturated
37
Saturated
very concentrated solution | any added solute will no longer be dissolved
38
Supersaturated
solute greater than that of a saturated solution
39
Solubility
ability of a solute to dissolve in a solvent
40
Heterogenous Mixture
components separate into distince phases
41
Suspension
Suspended particles tend to settle ad separate from the medium
42
Colloid
particles remain at afloat and never settle but can still be seen
43
Properties of Colloid
Tyndall Effect Brownian Movement Adsorption Electrical Property
44
Tyndall Effect
scattering of light
45
Brownian Movement
random movement of particles
46
Adsorption
adhesion of atoms, ions, or molecules to a surface
47
Separation Techniques
``` Filtration Distillation Crystallization Fractional Distillation Chromatography ```
48
Filtration
Insoluble solid | has Precipitate/Residue and Filtrate
49
Distillation
Solid in a liquid | obtains liquid through steam
50
Crystallization
Solid in a liquid | obtains the solid
51
Fractional distillation
two miscible liquid
52
Chromatography
mixture of small amount of solids
53
Postulates of Dalton's Atomic theory
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
Electron, e-
carries negative electric charge and found outside the nucleus of an atom
55
Proton, p+
carries positive electric charge ad found in the nucleus
56
Neutron, n^0
electrically neutral and found in the nuclues
57
Atomic Mass, A
number of protons + number of neutron
58
Atomic Number, Z
number of protons (in neutral atoms, this is equal to the number of electrons)
59
Ions
formed when atoms lose or gain electrons
60
Cations
positively charged ions, formed when an atom loses one or more electrons
61
Antions
negatively charged ions, forced then an atoms gain one or more electrons
62
Isotoped
atoms of the same elements with different number of neutrons and different atomic mass
63
Principle Quantum Number, n
denotes the shell or the main energy level in which the electron is found
64
Azimuthal Quantum number, l
denotes the subshell and determines the shape of the orbital
65
Magnetic Quantum number, ml
identifies the orbital where the electron is situated
66
Spin Quantum number, ms
determines the direction of the spin of the electron
67
Electron Configuration
number, distribution, or arrangement of electrons
68
Aufbau Principle
states that electrons fill up the lowest energy level first
69
Hund's Rule of Maximum Multiplicity
electrons occupy separate orbitals in the same subshell with parallel spins
70
Pauli's Exclusion Principle
no two electrons will have the same set of quantum numbers
71
Group/Family
``` 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
Period/Series
each horizontal row | the period number determines the ordinal value of the outermost shell
73
Classification of Elements
Metals Nonmentals Metalloids
74
Periodic Law
atoms of different elements are arranged in increasing atomic number, periodic properties are observed
75
Atomic Radius
size of an atom | distance from the nucleus to the outermost electron
76
Electronegativity
Tendency of a bonded atom to attract electrons in a covalent bond
77
Ionization Energy
the minimum energy required to remove an electron from the outermost shell of a gaseous atom
78
Electron Affinity
the energy released when a gaseous atoms gains an extra electron
79
Metallicity
describes properties such as conductivity, ductility, malleability
80
Chemical Bonds
Ionic Bounds Covalent : Polar and Nonpolar
81
Ionic Bounds
Losing (metal) and gaining (non-metal) of electrons
82
Covalent Bonds
sharing of electrons
83
Polar Covalent
partially positive and a slightly negative region between atoms unequal sharing of electrons (one is more electronegative than the other)
84
Non-polar Covalent
electrons are shared equally and present in homonuclear diatomic molecules

Review Classes - Science (6 decks)

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