Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

PSMA > Module 1 - Inorganic Chemistry > Flashcards

Module 1 - Inorganic Chemistry Flashcards

1
Q

Democritus Era

A

460-370 BC

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

ELECTRONS
Discovered by:
Mass:
Coulumb:
Charge:

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

PROTONS
Discovered by:
Mass:
Coulumb:
Charge:

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

NEUTRONS
Discovered by:
Mass:
Coulumb:
Charge:

A

James Chadwick 1932
1.67493 x 10-24
0
0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

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

A

corpuscles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Clouds of probability is called

A

Orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

ATOMIC STRUCTURE
Atoms are elliptical orbits of increasing number

A

RUTHERFORD-BOHR MODEL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

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

A

HEISENBURG UNCERTAINTY PRINCIPLE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
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”

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

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

A

 Pauli’s Exclusion Principle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

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

A

 Principal Quantum Number (n)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

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

A

Magnetic Quantum Number (m)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

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

A

Spin Quantum Number (s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

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

A

Hund’s Rule of Maximum Multiplicity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

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

A

ELECTRON CONFIGURATION THEORY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

○the values are from 0 to n - 1

A

Azithmuthal QN

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

the value range from -1 to +1

A

Magnetic Quantum Number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

1-4th Energy Level = Maximum number of electrons

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

equal to the number of protons and electrons

A

ATOMIC NUMBER (Z)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

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

A

MASS NUMBER (A)

32
Q

Nuclear notation

A

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

33
Q

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

A

ISOTOPES

34
Q

__ isotopes is usually present in greater abundance than another isotopes

A

one

35
Q

 atoms of different elements having the same number of neutrons

A

ISOTONES

36
Q

 atoms of different elements having the same atomic mass

A

ISOBARS

37
Q

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

A

IONS

38
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

39
Q

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

A

MOLECULES

40
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

41
Q

o positively charged electrodes

A

Anode

42
Q

can also be zero

A

WEIGHT

43
Q

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

A

1/6

44
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

45
Q

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

A
  1. Elements
46
Q

○ possess the characteristics of metals and non-metals

A

1.3 Metalloids

47
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%

48
Q

HUMAN BODY COMPONENTS AND %

A

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

49
Q

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

A

COMPOUNDS

50
Q

○ formed when there is a transfer of e-

A

2.1 Ionic compound

51
Q

○ formed when e- are shared

A

2.2 Covalent compound

52
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

53
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

54
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

55
Q

ACID-BASE THEORY
(Proponent + Theory)

A

Arrhenius
Bronsted-Lowry
Lewis

56
Q

Water when it loses a proton forms ____

A

hydroxide ion

57
Q

Water when it accepts a protn forms ____

A

hydronium ion

58
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

59
Q

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

A

BUFFERS

60
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

61
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

62
Q

acid and bases with a product of salt and water

A

○ NEUTRALIZATION

63
Q

○ substances that consists oxygen and other elements

A

2.5.4 Oxides

64
Q

blue litmus paper to red

A

ACID

65
Q

red litmus paper to blue

A

BASE

66
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

67
Q

Solution particle size

A

< 10 ^(-7)cm

68
Q

Colloid particle size is

A

10-7 cm and 10-5 cm

69
Q

Suspension particle size is

A

> 10 ^(-5) cm

70
Q

 the liquids are colloidally suspended in another liquid samples

A

EMULSIONS

71
Q

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

A

colloids

72
Q
  • is the scattering of light by particles in a colloid or suspension
A

TYNDALL EFFECT

73
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

74
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

75
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

76
Q

aka Proust’s Law

A

LAW OF DEFINITE PROPORTIONS

77
Q

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

A

LAW OF COMBINING WEIGHTS

PSMA (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions