Module 1 (Basic concept of inorganic chemistry) Flashcards
1
Q
it occupies space and mass
A
matter
2
Q
group of matter with the same properties
A
state of matter
3
Q
arranged in regular repeating pattern
A
solid
4
Q
reaction happen when it vibrates
A
solid
5
Q
no definite shape and flows easily
A
liquid
6
Q
its atom is more free compared to solid
A
liquid
7
Q
its atom/ molecules fly in all direction at great speed
A
gas
8
Q
attractive forces are insignificant as they are far apart
A
gas
9
Q
contains protons and electrons
A
plasma
10
Q
loses electron at very high temperature
A
plasma
11
Q
result of the mixture of electron and nuclei
A
plasma
12
Q
combination of 2 or more substances wherein their distinct properties are still the same
A
mixture
13
Q
air, cement, milk, coffee, and softdrinks
A
mixture
14
Q
have definite and constant composition and distinct properties
A
pure substances
15
Q
ethanol, table salt, carbon dioxide, water and silver
A
pure substances
16
Q
homogeneous and heterogeneous
A
mixture
17
Q
composition of the mixture is the same through out the solution
A
homogeneous mixture
18
Q
composition of the mixture is not uniform
A
heterogeneous
19
Q
substance that cannot be broken down into smaller substance by chemical means
A
element
20
Q
combination of 2 or more element
A
compound
21
Q
can be observed or measured
A
physical properties
22
Q
have chemical changed
A
chemical properties
23
Q
boiling point, freezing point, color, shape, and odor
A
physical properties
24
Q
boiling, freezing, acidity and flammability
A
chemical properties
25
something you can measure
extensive property
26
quality of compound
intensive property
27
weight, height, length, and distance
extensive property
28
does not result in new substance
physical change
29
result to a new substance
chemical change
30
freezing, boiling, and bending
physical change
31
rust in a nail and burning of paper
chemical change
32
measured quantity written in numbers
measurement
33
can bee seen directly or can be seen through naked eye
macroscopic property
34
cannot be seen directly
microscopic
35
basic unit of an element
atom
36
in 15th century he proposed that matter is made up of small particles called atomos
Democritus
37
in 1704 he proposed a mechanical universe with small solid masses in motion
Isaac Newton
38
in 1808 proposed the Atomic Theory with spherical solid atoms based upon measurable properties of mass
John Dalton
39
1. Each element is composed of a small particle which is called atom
2. all atoms of an element is identical, having the same size, mass and chemical properties. the atom of an element is different from the atom of all elements
3. compound is made up of one atom of more than 1 element
4. chemical reaction involves only separation, recombination, and rearrangement of atom. it does not result in their creation or destruction
Atomic Theory
40
in 1911 he proposed the planetory or nuclear model of atom
Ernest Rutherford
41
revealed 3 types of radiation, alpha, beta, and gamma
Ernest Rutherford
42
in 1908 he conducted an oil drop experiment to determine the charge on the electron and proton
Robert Millikan
43
In 1869 he discovered Radioactivity
Henri Becquerel
44
Father of Modern Atomic and Nuclear Physics
Henri Becquerel
45
in 1922 he developed an explanation on atomic structure which underlies the regulatory of the periodic table
Neils Bohr
46
in 1923 he discovered that electron have dual nature - similar to particles and waves
Louis De Broglie
47
in 1927 he proposed the principle of indeterminacy
Werner Heisenberg
48
in 1930 he viewed electron as a continuous cloud and introduced the Wave Mechanics as a mathematical model of atom
Erwin Schrodinger
49
he proved the existence of neutrons
James Chadwick
50
number of proton in the nucleus of an atom of an element
atomic number
51
the number of protons is equal to the number of electrons
neutral atom
52
total number of protons and neutron present in the nucleus of an atom of an element
mass number
53
atoms of the same atomic number but different mass number and different number of neutrons
isotopes
54
something is the same, something is different
Iso
55
protium, deuterium, and tritium
hydrogen isotopes
56
required to describe the distribution of electrons
quantum numbers
57
Describe the energy of electrons
1-3 quantum no. (Principal, Angular momentum, and Magnetic quantum number)
58
describe the direction of motion of electrons
4th quantum no. (Spin quantum number)
59
as the n+1 value increases, the energy of electrons also increases
N1+ rule
60
the number of electrons is equal to the atomic number. the electron added will enter the orbitals in the order of increasing energy. orbitals cannot take more than 2 electrons.
Aufbau Principle
61
every orbitals in a sub shell is singly occupied with one electron before every other orbitals are doubly occupied.
Hunds rule of maximum multiplicity
61
chart of elements with the same physical and chemical properties are grouped together
periodic table
62
vertical line or row in the periodic table (lanthanides and actinides)
period
63
causes the energy of 2 atom close together to be markedly lower
chemical bond
63
attraction between 2 or more atoms that allows them to be able to create a stable new compound
chemical bond
64
combination of metal and nonmetal
ionic compound
65
involves the transfer of electrons
ionic bond
65
combination of 2 non-metal
molecular compound
66
movement of protons in the sea of electrons
metallic bond
66
involves the sharing of 2 electron of 2 atoms
covalent bond
67
68
2 or more substance are combined to form a new product
combination reaction
69
opposite of combination reaction
decomposition reaction
70
one element replaces one similar element in a compound
single replacement reaction
71
reaction in which positive and negative ions of 2 ionic compounds exchange places to form 2 new compounds
double replacement reaction
71
gain electrons and the oxidation number decreases
reduced half
71
loses electron and the oxidation number increases
oxidized half
72
oxidation is loss
reduction
73
oxidation is gain
oxidation
73
loss of electron (LEO)
oxidation
74
gain of electron (GER)
reduction
75
a section of chemistry that involves using the relationship between reactants and products in a chemical equation to determine the desired quantitative data
stoichiometry
76
means element
stoikhein
77
means measure
metron
78
numbers we use to determine if the equation is balance
stoichiometric coefficients
79
Change that involve the change in intensive property
Chemical change
80
Change thay envolve energy, the endothermic and exothermic
Chemical change
