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PSMA > Module 1 - Inorganic Chemistry > Flashcards

Module 1 - Inorganic Chemistry Flashcards

1
Q

Democritus Era

A

460-370 BC

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2
Q
A
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3
Q

ELECTRONS
Discovered by:
Mass:
Coulumb:
Charge:

A

Joseph John Thomson
9.10938 x 10-28
-1.6022 x 10 -19
-1

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4
Q

PROTONS
Discovered by:
Mass:
Coulumb:
Charge:

A

Eugene Goldstein
1.67262 x 10-24
+1.6022 x 10 -19
+1

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5
Q

NEUTRONS
Discovered by:
Mass:
Coulumb:
Charge:

A

James Chadwick 1932
1.67493 x 10-24
0
0

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6
Q

In 1897, J.J. Thomson discovered electrons which he named ______

A

corpuscles

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7
Q
  • It shows the atom as composed of electrons scattered throughout a spherical cloud of positive charge
    -Recognize electrons as components of atoms
    -No nucleus, didn’t explain
A

Plum Pudding Model
Joseph John Thomson
1904

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8
Q

-His theory stated that atoms are indivisible, those of a given
Elements are identical, and compounds are combinations of different types of atoms
- Recognized atoms of a particular element differ from to other
-Atoms are not indivisible, composed of subatomic particles

A

SOLID SPHERE MODEL
(JOHN DALTON 1803)

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9
Q

-Fired positively charged alpha particles at a thin sheet of gold foil. Most passed through with a little deflection, but some
deflected at large angles

-This was only possible if the atom was mostly empty space, with
a positive charge concentrated in the center: the nucleus

-Realize positive charge was localized in the nucleus of an atom

-Did not explain why electrons remain in orbit around the nucleus

A

NUCLEAR MODEL (ERNEST RUTHERFORD 1911)

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10
Q

-Modified rutherford’s model of the atom by stating that electrons move around the nucleus in orbits of fixed sizes and
energies.

-Electron energy in this model was quantized; electrons
could not occupy values of energy between the fixed energy
levels

-Proposed stable electron orbits explain the emission spectra of some elements

-Moving electrons should emit energy and collapse into the nucleus, model did not work well for heavier atoms

A

PLANETARY MODEL
(Neils Bohr 1913)

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11
Q

Proponent stated that electrons do not move in set paths around the nucleus, but in waves. It is impossible to know the
exact location of the electrons; instead, you have clouds of probability called orbitals, in which we are more likely to find an electron

Shows electrons didn’t move around the nucleus in orbits but in clouds where their position is uncertain

Still widely accepted as most accurate model of the atom

A

QUANTUM MODEL (ERWIN SCHRODINGER 1926)

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12
Q

Clouds of probability is called

A

Orbitals

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13
Q

ATOMIC STRUCTURE
Atoms is a spherical mass containing electrons and that this spherical mass is positive but is made neutral by the electrons embedded in it.

Aka Plum Pudding Model

A

THOMSON MODEL

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14
Q

ATOMIC STRUCTURE
In this model, protons are in the nucleus and the electrons are in
the orbital motion around the nucleus  Electrons may be found in any several definite orbits around the
nucleus

A

BOHR MODEL OF AN ATOM

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15
Q

ATOMIC STRUCTURE
Atoms are elliptical orbits of increasing number

A

RUTHERFORD-BOHR MODEL

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16
Q

This principle states that simultaneous determination of the exact position and exact momentum of electron is impossible

A

HEISENBURG UNCERTAINTY PRINCIPLE

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17
Q

Aka Electron Cloud Model

 In this model, the nucleus is a single cluster of particles at the center of the atom while the electrons are everywhere

 Has dense positive charge nucleus at the center and electrons still have a distinct amount of energy which are usually place outside the nucleus

 The electrons are not orbiting the nucelus in definite or fixed pathways. Instead of orbiting, the electrons are placed in orbitals outside the nucleus (electrons are still orbiting the nucelus but not in fixed pathways)

A

WAVE MECHANICAL ATOM

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18
Q

 This theory makes the assertion that electromagnetic radiation like X-rays, gamma rays, radio waves and light rays are made up of small bits of energy

A

SCHRODINGER “QUANTUM MODEL”

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19
Q

states that no two electrons can have the same set of quantum numbers

A

 Pauli’s Exclusion Principle

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20
Q

○ corresponds to main energy levels
○ described the size of the orbital

A

 Principal Quantum Number (n)

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21
Q

or angular momentum quantum number (can give and measure angular momentum of an electron and its motion around the nucleus)
○described the shape of orbital

A

Azithmuthal Quantum Number (l)

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22
Q

○indicate the behavior of electrons in the magentic field
○described the orientation in space of a particular orbital

A

Magnetic Quantum Number (m)

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23
Q

○indicate the spin of an electron about its own axis in clockwise or counterclockwise

A

Spin Quantum Number (s)

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24
Q

ATOMIC STRUCTURE
This theory states that the number of orbital types in a given shell is equal to the shell number

Orbitals have a three-dimensional region in space where the probability of finding the electron is greatest

A

ORBITAL THEORY

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25
Q

○orbitals with the same electron of same energy level must be filled in singly before pairing

A

Hund’s Rule of Maximum Multiplicity

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26
Q

ATOMIC STRUCTURE
According to this theory:
1st - 4th main energy level

A

ELECTRON CONFIGURATION THEORY

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27
Q

states that atoms may be built by progressively filling the main energy levels, sub levels and orbitals with electrons according to increasing level

*** levels of lower energy level are occupied first

A

AUFBAU PRINCIPLE

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28
Q

○the values are from 0 to n - 1

A

Azithmuthal QN

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29
Q

the value range from -1 to +1

A

Magnetic Quantum Number

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30
Q

1-4th Energy Level = Maximum number of electrons

A

1st = 2e
2nd = 8e
3rd = 18e
4th = 32e

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31
Q

equal to the number of protons and electrons

A

ATOMIC NUMBER (Z)

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32
Q

total number of protons and neutrons on the nucleus of nucleons,

A

MASS NUMBER (A)

33
Q

Nuclear notation

A

 A (Mass number)
 N (Neutrons)
 Z (Atomic number)
 X (Element)

34
Q

 in other words, they have the same number of protons and electrons but different number of neutrons

A

ISOTOPES

35
Q

__ isotopes is usually present in greater abundance than another isotopes

A

one

36
Q

 atoms of different elements having the same number of neutrons

A

ISOTONES

37
Q

 atoms of different elements having the same atomic mass

A

ISOBARS

38
Q

 it is a charged species, an atom or a molecule, that has lost or gained one or more electrons

A

IONS

39
Q

 it is the smallest indivisible portion of a pure chemical substance that has its unique set of chemical properties, that is, its potential to undergo a certain set of chemical reactions with other substances

A

MOLECULES

40
Q

 aggregates of at least two atoms in a definite arrangement and held together by chemical forces

A

MOLECULES

41
Q

 a conductor that is used to make contact with non-metallic part of a circuit
 commonly used in electrochemical cells, semi-conductors such as diodes and other medical devices

A

ELECTRODES

42
Q

o positively charged electrodes

A

Anode

43
Q

can also be zero

A

WEIGHT

44
Q

when travelled to the moon, the weight of an object will only be ___ of its weight on earth

A

1/6

45
Q

are made up only of one kind of matter possessing a definite, fixed and unvarying compositions
has unique set of properties

A

PURE SUBSTANCES

46
Q

○ simplest form of substance that cannot be decomposed by chemical means; building blocks of matter

A
  1. Elements
47
Q

○ possess the characteristics of metals and non-metals

A

1.3 Metalloids

48
Q

EARTH’S CRUST COMPONENTS & %

A

Oxygen - 45.5%
Silicon - 27.2%
Aluminum - 8.3%
Iron - 6.2%
Others - 5.3%
Calcium 4.7%
Magnesium 2.8%

49
Q

HUMAN BODY COMPONENTS AND %

A

Oxygen - 65%
Carbon - 18%
Hydrogen - 10%
Nitrogen - 3%
Calcium - 1.6%
Phosphorus - 1.2%
Others - 1.2%

50
Q

○ are substances whose molecules are made up of two or more kinds of atoms
○ combined in definite proportion

A

COMPOUNDS

51
Q

○ formed when there is a transfer of e-

A

2.1 Ionic compound

52
Q

○ formed when e- are shared

A

2.2 Covalent compound

53
Q

○ formed by interaction between elements which are usually metallic but the resulting compound behaves just like an ordinary metal

A

2.3 Metallic compound

54
Q

○ any of the large class of chemical compounds in which one or more atoms of carbons are covalently linked to the atoms of another elements
○ carbon-containing compounds (such as H, O, N) except carbides, carbonates, and cyanides

A

2.4 Organic compound

55
Q

○ these are combined with definite proportions of two elements
○ do not contain carbon
○ eg. graphites, carbon dioxide, and carbon monoxide

A

2.5 Inorganic compound

56
Q

ACID-BASE THEORY
(Proponent + Theory)

A

Arrhenius
Bronsted-Lowry
Lewis

57
Q

Water when it loses a proton forms ____

A

hydroxide ion

58
Q

Water when it accepts a protn forms ____

A

hydronium ion

59
Q

based on electrolytes nature; an equation that will provide the starting point for modern treatments of non- ideality of electrolytes solution

++ proponents

A

DEBYE-HUCKEL THEORY | by Peter Debye and Erich Huckel

60
Q

substances that are resistant to pH; apply the theory of Henderson-Hasselbach equation

A

BUFFERS

61
Q

maximum amount of either the strong acid or the strong base that can be added before a significant change in the pH will occur; apply the Van Slyke Equation

A

BUFFER CAPACITY

62
Q

○ combination of any positive ion and negative ion except for OH; formed by the combination of acids and bases

A

2.5.3 Salts

63
Q

acid and bases with a product of salt and water

A

○ NEUTRALIZATION

64
Q

○ substances that consists oxygen and other elements

A

2.5.4 Oxides

65
Q

blue litmus paper to red

A

ACID

66
Q

red litmus paper to blue

A

BASE

67
Q

Define the pH levels of:
Strong acids
Weak acids
Neutral
Weak bases
Strong bases

A

pH 1-3 pH 4-6 pH 7 pH 8-10 pH above 11

68
Q

Solution particle size

A

< 10 ^(-7)cm

69
Q

Colloid particle size is

A

10-7 cm and 10-5 cm

70
Q

Suspension particle size is

A

> 10 ^(-5) cm

71
Q

 the liquids are colloidally suspended in another liquid samples

A

EMULSIONS

72
Q

The particle size of ____ are much larger than solution but smaller than suspensions

A

colloids

73
Q
  • is the scattering of light by particles in a colloid or suspension
A

TYNDALL EFFECT

74
Q

-aka Proust’s Law
-a given chemical compound will always contains the same elements in the same proportion by mass

A

LAW OF DEFINITE PROPORTIONS

75
Q

-when two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of a small whole numbers

A

LAW OF MULTIPLE PROPORTIONS

76
Q

elements combine in the ratio of their combining weights or chemical equivalents; or in some simple multiple or sub-multiple of that ratio.

A

LAW OF COMBINING WEIGHTS

77
Q

aka Proust’s Law

A

LAW OF DEFINITE PROPORTIONS

78
Q

 also called the Law of Reciprocal Proportions or Law of Equivalents

A

LAW OF COMBINING WEIGHTS

PSMA (15 decks)

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