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INORGANIC CHEMISTRY > PICLEC: MODULE 1 > Flashcards

PICLEC: MODULE 1 Flashcards

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1
Q

The science that describes matter—its properties, the changes it undergoes, and the energy changes that accompany those processes

A

CHEMISTRY

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2
Q

The CENTRAL SCIENCE

A

CHEMISTRY

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3
Q

Branches of Chemistry

A
  1. ORGANIC CHEMISTRY
  2. INORGANIC CHEMISTRY
  3. ANALYTICAL CHEMISTRY
  4. BIOCHEMISTRY
  5. PHYSICAL CHEMISTRY
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4
Q

BRANCH OF CHEMISTRY
- Hydrocarbons and its derivatives

A

ORGANIC CHEMISTRY

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5
Q

BRANCH OF CHEMISTRY
- Inorganic compounds, metals, minerals

A

INORGANIC CHEMISTRY

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6
Q

BRANCH OF CHEMISTRY
- Detection and identification of substances present (qualitative analysis) or amount of each substance (quantitative analysis)

A

ANALYTICAL CHEMISTRY

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7
Q

BRANCH OF CHEMISTRY
- Processes in living organisms

A

BIOCHEMISTRY

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8
Q

BRANCH OF CHEMISTRY
- Behavior of matter

A

PHYSICAL CHEMISTRY

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9
Q

Anything that has mass and occupies space; is tangible

A

MATTER

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10
Q

Measure of the quantity of matter

A

MASS

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11
Q

Amount of space

A

VOLUME

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12
Q

The capacity to do work or to transfer heat

A

ENERGY

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13
Q

TYPES OF ENERGY:

A
  1. KINETIC ENERGY
  2. POTENTIAL ENERGY
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14
Q

TYPES OF ENERGY
- Energy in motion

A

KINETIC ENERGY

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15
Q

TYPES OF ENERGY
- Energy at rest

A

POTENTIAL ENERGY

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16
Q

ENERGY CHANGES:

A
  1. EXOTHERMIC
  2. ENDOTHERMIC
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17
Q

ENERGY CHANGES
- Release (heat)

A

EXOTHERMIC

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18
Q

ENERGY CHANGES
- Absorbs (heat)

A

ENDOTHERMIC

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19
Q

STATES OF MATTER

A
  1. SOLID
  2. LIQUID
  3. GAS
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20
Q

STATES OF MATTER
- Molecules packed close together orderly; Rigid

A

SOLID

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21
Q

STATES OF MATTER
- Molecules are close but randomly arranged; Flows and assumes shape of container

A

LIQUID

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22
Q

STATES OF MATTER
- Molecules are far apart; Fills any container
completely

A

GAS

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23
Q

CHANGES OF STATES

A

S - L = MELTING
L - S = FREEZING

L - G = BOILING
G - L = CONDENSATION

G - S = DEPOSITION
S - G = SUBLIMATION

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24
Q

Can be observed or measured without changing the identity of the substance.

e.g. color, hardness, melting point, boiling point

A

PHYSICAL PROPERTIES

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25
Q

Exhibited by matter as it undergoes changes in
composition.

e.g. hydrogen has the potential to ignite and explode given the right conditions
e.g. iron reacts with oxygen gas to form rust

A

CHEMICAL PROPERTIES

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26
Q

Dependent on the amount of substance.

e.g. MASS – more substance, greater mass
e.g. VOLUME – more substance, greater volume

A

EXTENSIVE PROPERTIES

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27
Q

Independent on the amount of substance

e.g. DENSITY, Electrical Conductivity

A

INTENSIVE PROPERTIES

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28
Q

Way to Tell Intensive and Extensive Properties Apart

A

▪ Take two identical samples of a substance and put them
together.
▪ If this doubles the property (e.g., twice the mass, twice as
long), it’s an extensive property.
▪ If the property is unchanged by altering the sample size,
it’s an intensive property.

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29
Q
  • one or more substances are used up
  • one or more new substances are formed,
  • energy is absorbed or released
  • IRREVERSIBLE
  • e.g. burning of paper, cooking an egg, souring of milk
A

CHEMICAL CHANGE

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30
Q
  • no change in chemical composition
  • REVERSIBLE
  • e.g. shredding paper, boiling of water, breaking a
    bottle
A

PHYSICAL CHANGE

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31
Q

Variable Composition (e.g. 70%, 80% or 95% ethanol in water)

May be separated into pure substances by physical methods (e.g. distillation, filtration)

A

MIXTURE

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32
Q

Fixed composition (e.g. 100% ethanol)

Cannot be separated into simpler substances by physical methods

A

PURE SUBSTANCE

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33
Q
  • Components are NOT distinguishable (single phase)
  • Have same composition throughout (i.e. same amount
    in any areas)
  • e.g. SOLUTION
A

HOMOGENEOUS MIXTURE

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34
Q
  • Components are distinguishable (multiple phases)
  • Do NOT have same composition throughout (i.e.
    different amount in various areas)
  • e.g. SUSPENSION
A

HETEROGENEOUS MIXTURE

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35
Q
  • Can be decomposed to simpler substance by
    chemical changes
  • consists of atoms of two or more different elements
    bound together.
  • e.g. water, H2O can be broken into hydrogen and
    oxygen gases via electrolysis
A

COMPOUND

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36
Q
  • Cannot be decomposed to simpler substance by chemical changes
  • Consists of only one kind of atom
A

ELEMENTS

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37
Q
  • The smallest unit that retains the properties of an element.
A

ATOM

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38
Q
  • All matter is composed of atoms and these cannot be made or destroyed.
A

DALTON’S THEORY

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39
Q

The number of protons in the nucleus of
an atom determines its identity; this
number is known as the atomic number
of that element.

e.g.
- Hydrogen atom contains 1 proton.
- Lithium atom contains 3 protons.

A

ATOMIC NUMBER (Z)

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40
Q

The mass number of an atom is the sum of the number of
protons and the number of neutrons in its nucleus; that is

𝑴𝒂𝒔𝒔 𝑵𝒖𝒎𝒃𝒆𝒓 = # 𝒐𝒇 𝒑 + # 𝒐𝒇 𝒏

𝑴𝒂𝒔𝒔 𝑵𝒖𝒎𝒃𝒆𝒓 = 𝑨𝒕𝒐𝒎𝒊𝒄 𝑵𝒖𝒎𝒃𝒆𝒓 + 𝑵𝒆𝒖𝒕𝒓𝒐𝒏 𝑵𝒖𝒎𝒃𝒆𝒓

A

MASS NUMBER (A)

41
Q

Isotopes are atoms of the SAME ELEMENT with DIFFERENT MASSES

They are atoms containing the same number of protons but different numbers of neutrons.

A

ISOTOPES

42
Q

Represents the composition of the nucleus

A

NUCLIDE SYMBOL

43
Q

SAME MASS NUMBER - DIFFERENT ATOMIC NUMBER

A

ISOBARS

44
Q

SAME NEUTRONS - DIFFERENT ATOMIC NUMBER

A

ISOTONES

45
Q

Many elements occur in nature as mixtures of isotopes.

The atomic weight of such an element is the weighted average of the masses of its isotopes.

Atomic weights are fractional numbers, not integers.

A

ATOMIC WEIGHT

46
Q
  • Greek word “Atomos” – uncuttable
  • Atom as solid indivisible sphere
A

LEUCIPPUS AND DEMOCRITUS

47
Q
  • Matter is made up of four elements
A

ARISTOTLE AND OTHERS

48
Q
  • Solid Sphere (Billiard Ball) Model
  • Atom as solid sphere but
    NOT indivisible
A

DALTON’S ATOMIC THEORY
JOHN DALTON

49
Q

DISCOVERY OF ELECTRONS

A

▪ Elements of a chemical compound are held together by
electrical forces.
- Humphry Davy (1800s)
▪ Relationship between the amount of electricity used in
electrolysis and the amount of chemical reaction that
occurs.
- Michael Faraday (1832)
▪ “Electrons” → Electric ions
- George Stoney (1891)

50
Q

Elements of a chemical compound are held together by
electrical forces.

A

HUMPHRY DAVY

51
Q

Relationship between the amount of electricity used in electrolysis and the amount of chemical reaction that occurs.

A

MICHAEL FARADAY

52
Q

“Electrons” → Electric ions

A

GEORGE STONEY

53
Q

The Discovery of Electrons

A
  1. CATHODE RAY TUBE
  2. OIL- DROP EXPERIMENT
  3. SATURN LIKE MODEL
54
Q

The Discovery of Electrons
- Joseph John Thomson (1897)
- Most convincing evidence of electrons
- Plum pudding model

A

CATHODE-RAY TUBE EXPERIMENT

55
Q

The Discovery of Electrons
- Robert Millikan (1909)
- Determine the charge of electrons

A

OIL-DROP EXPERIMENT

56
Q

The Discovery of Electrons
- Hantaro Nagaoka (1903)

A

SATURN-LIKE MODEL

57
Q

The Discovery of Protons

A
  1. CANAL RAYS EXPERIMENT
  2. SCATTERING EXPERIMENT
  3. NUCLEAR MODEL
58
Q

The Discovery of Protons
- Eugen Goldstein (1886)
- Cathode-ray tube also generates a stream of
positively charged particles
- These positive rays, or positive ions, are created
when the gaseous atoms in the tube lose electrons.

A

CANAL RAYS EXPERIMENT

59
Q

The Discovery of Protons
- Ernest Rutherford (1910)

Assumption:
- If the Thomson model of the atom were correct, any
alpha-particles passing through the foil would have
been deflected by very small angles.
- Quite unexpectedly, nearly all of the a-particles
passed through the foil with little or no deflection.

Rutherford’s Conclusion:
- Atoms consist of very small, very
dense positively charged nuclei
surrounded by clouds of electrons
at relatively large distances from
the nuclei.

A

SCATTERING EXPERIMENT

60
Q

The Discovery of Protons
- Positive charge localized in the NUCLEUS

A

NUCLEAR MODEL

61
Q

The Discovery of Neutrons

A
  1. BOHR’ S MODEL
    - BOHR’S PLANETARY MODEL
62
Q

The Discovery of Neutrons
- Each orbit thus corresponds to a definite energy level
for the electron.
- When an electron is excited from a lower energy level
to a higher one, it absorbs a definite (quantized)
amount of energy.
- Electrons occupy only certain energy levels in atoms.

A

BOHR’S PLANETARY MODEL

63
Q

Studied X-rays given off by various
elements.

A

H.G.J. MOSELEY

64
Q

Bombardment of beryllium with high-energy alpha-particles produced NEUTRONS

A

JAMES CHADWICK

65
Q

Described the electron of a hydrogen atom as revolving around its nucleus in one of a discrete set of circular orbits.

A

NIELS BOHR

66
Q
  • Proposed the idea of wave-like nature of electrons
    ▪ Electrons can be treated as waves more effectively than
    as small compact particles traveling in circular or elliptical
    orbits.
A

LOUIS DE BROGLI

67
Q

Based on the wave properties of matter

A

QUANTUM MECHANICS

68
Q
  • For electrons, it is not possible to determine the exact momentum and the exact position at the same moment in time.
A

WERNER HEISENBERG’S UNCERTAINTY PRINCIPLE

69
Q

It estimates the position of electrons and quantifies energy levels.

A

ERWIN SCHRÖDINGER’S WAVE EQUATION

70
Q

A region of space in which the probability of finding an electron is high.

A

ATOMIC ORBITALS

71
Q

Erwin Schrödinger
- Electron Cloud Model
- Quantum Mechanical Model

A

MODERN ATOMIC MODEL

72
Q

QUANTUM NUMBERS

A
  1. Principal QN (𝒏)
  2. Orbital QN (𝒍)
  3. Magnetic QN (𝒎𝒍)
  4. Spin QN (𝒎𝒔)
    - for individual electrons only
73
Q

▪ 𝒏 = 𝟏, 𝟐, 𝟑, … (𝒏)
▪ Orbital → SHELL or ENERGY LEVEL
▪ Distance of the electron
from the nucleus
▪ Higher 𝒏, higher energy

A

PRINCIPAL QUANTUM NUMBER (n)

74
Q

▪ a.k.a. Azimuthal or Orbital Angular momentum Quantum
Number
▪ 𝒍 = 𝟎, 𝟏, 𝟐, 𝟑, … (𝒏 − 𝟏)
▪ Orbital → SUBSHELL/ SUBLEVEL
▪ Shape of the orbital
- 𝒍 = 𝟎 s spherical
- 𝒍 = 𝟏 p dumb-bell
- 𝒍 = 𝟐 d clover leaf
- 𝒍 = 𝟑 f complex

A

ANGULAR/ORBITAL MOMENTUM QUANTUM NUMBER

75
Q

▪ 𝒎𝒍 = −𝒍 … 𝟎 … + 𝒍
▪ Orbital → Specific orbital
▪ Orientation in space of the orbital

A

MAGNETIC QUANTUM NUMBER

76
Q

▪ For each INDIVIDUAL ELECTRON only
▪ 𝒎𝒔 = + 𝟏/𝟐 , - 𝟏/𝟐
▪ Direction of spin (clockwise or counter-clockwise)
▪ Quantum Number and Electron Configuration

A

SPIN QUANTUM NUMBER

77
Q

▪ “Distribution of electrons”
▪ describes the number and arrangement of electrons in
orbitals, subshells and shells in an atom.
▪ Ground state
- Atom in its lowest energy, or unexcited, state.

A

ELECTRON CONFIGURATION

78
Q
  • Orbitals fill in order of increasing energy, from lowest to highest.
A

AUFBAU PRINCIPLE

79
Q
  • No more than two electrons can occupy each orbital, and if two electrons are present, they must have opposite spins.
A

PAULI EXCLUSION PRINCIPLE

80
Q
  • The order of fill is the same but as you can see from
    above the electrons are placed singly into the boxes
    before filling them with both electrons.
  • A single electron will occupy an empty orbital first
    before pairing.
A

HUND’S RULE

81
Q

Arranged the periodic table based on chemical properties

A

DIMITRI MENDELEEV

82
Q

Arranged the periodic table based on physical properties

A

LOTHAR MEYER

83
Q

▪ Both emphasized the periodicity, or regular periodic
repetition of properties with increasing atomic weight.

A

DIMITRI MENDELEEV AND LOTHAR MEYER

84
Q
  • “The properties of the elements are periodic functions
    of their atomic numbers.”
    ▪ Vertical Columns → Groups or Families
    ▪ Horizontal Rows → Periods
A

PERIODIC LAW

85
Q

High electrical conductivity that decreases with increasing temperature

A

METALS

86
Q

High thermal conductivity

A

METALS

87
Q

Malleable, Ductile, silver luster, forms cat ions by losing electrons, form ionic compounds with non metals, solid state characterized by metallic bonding

A

METALS

88
Q

Poor electrical conductivity

A

NON METALS

89
Q

Good heat insulators

A

NON METALS

90
Q

Brittle, non-ductile, no metallic luster, form anions by gaining electrons, form ionic compounds with metals and molecular compounds with non metals, covalently bonded molecules

A

NON METALS

91
Q
  • Show some properties that are characteristic of both
    metals and non-metals
  • Semiconductors
    ▪ insulators at lower temperatures but become
    conductors at higher temperatures
    ▪ silicon, germanium, and antimony
A

METALLOIDS

92
Q

PERIODIC PROPERTIES OF ELEMENTS
- Defined as half of the distance between the nuclei of neighbouring atoms in the pure element
- Expressed in Angstroms (1Å = 10-10 m)

A

ATOMIC RADII (size)

93
Q

PERIODIC PROPERTIES OF ELEMENTS
- The energy required to remove an electron from a gas-phase atom

A

IONIZATION ENERGY (IE)

94
Q

PERIODIC PROPERTIES OF ELEMENTS
- The energy change that occurs when an electron is attached to an atom in the gas phase to form an negative ion

A

ELECTRON AFFINITY (EA)

95
Q

PERIODIC PROPERTIES OF ELEMENTS
- Measure of the relative tendency of an atom to attract electrons to itself when it is chemically combined with another atom

A

ELECTRONEGATIVITY (EN)

96
Q

same mass no. different atomic no.

A

ISOBARS

97
Q

same elements different mass no.

A

ISOTOPES

98
Q

same neutrons different atomic no.

A

ISOTONES

INORGANIC CHEMISTRY (19 decks)

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