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Part 2 Science Flashcards

1
Q

anything that occupies space and has mass

A

MATTER

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2
Q
  • are homogenous materials with definite chemical properties and consists of
    one particular kind of matter.
A

PURE SUBSTANCES

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3
Q
  • is a substance that can no longer be decomposed into simpler ones by ordinary
    physical and chemical methods. There are at present 103 elements known. Of these, about 75
    are metals and the remaining constitutes the non metals and the metalloids.
A

ELEMENT

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4
Q

How many elements are present?
How many metals are there?

A

103
75

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5
Q

During ordinary chemical changes, elements remain uncharged. However, not it is possible to
decompose or change an element into another by extraordinary methods. Some radioactive
elements like _____and ______ spontaneously decompose or disintegrate.

A

Radium and Uranium

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6
Q

CLASSIFICATION OF ELEMENT

A

Metal, Non-metal, Metalloid

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7
Q

-Base forming elements whose atoms can lose electrons and form positive ions. The
nomenclature commonly ends “ium” or “um”

A

Metals

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8
Q

Properties of Metals

A

a. usually solid (except Hg)
b. opaque, lustrous
c. malleable
d. ductile
e. conductors of heat and electricity
f. usually heavy except for a few

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9
Q

Examples of metals

A

Ca, Al, Na, Fe, Ag

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10
Q
  • are acid forming elements whose atoms can gain electrons and form negative ions.
    The names usually end in “gen” “ine” “on”.
A

Non-Metal

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11
Q

Properties of Non Metal

A

a. usually gases of brittle solid (except bromine)
b. mostly transparent
c. light
d. poor conductors of heat and electricity

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12
Q

l, Cl, H, He, Ru,

A

Non-Metal

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13
Q

Examples of Non-Metal

A

Examples: l, Cl, H, He, Ru,

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14
Q
  • those elements which exhibit both metallic and non metallic properties.
A

Metalloids

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15
Q

Examples of metalloids

A

Examples
are antimony and arsenic

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16
Q
  • composed of two or more elements chemically combined in a definite
    proportion by weight
A

COMPOUND

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17
Q

Types of Compound

A

Organic
Inorganic

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18
Q
  • any member of a large class of chemical compounds whose molecules
    contain carbon
A

Organic compound

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19
Q
  • any compound that does not contain carbon.
A

Inorganic compound

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20
Q
  • compounds of oxygen and other elements
A

Oxides
*Inorganic

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21
Q

– compounds which contain hydrogen ions replaceable by metals. Example HCl, H2SO4,
HNO3

A

Acids
*Inorganic

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22
Q

– hydroxides of metals. Ex. NaOH. KOH

A

Bases
*Inorganic

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23
Q

– compounds which contain the negative radical of an acid and the positive radical of a
base

A

Salts
*Inorganic

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24
Q

Examples of inorganic

A

Ex. NaCl. CaBr2, CuSO4, Mg3(PO4)2

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25
Have definite composition
Compound
26
Have variable composition
Mixture
27
Always homogeneous
Compound
28
Maybe homogeneous or heterogeneous
Mixtures
29
Have definite properties
Compound
30
Have variable properties depending on the amount of components
Mixtures
31
The constituents are chemically combined
Compound
32
The components are not chemically combined
Mixtures
33
The constituents may be separated only by chemical means
Compound
34
the components may be separated by physical or chemical means
Mixtures
35
Constituents are the particles that composed a _______
compound
36
Components are the particles that composed a _______
mixture
37
composed of two or more substances in a variable composition
Impure substance or mixtures
38
Mixtures are classified into:
Homogeneous Heterogeneous
39
- composed of uniform composition and made up of only one phase
Homogeneous mixture
40
– a molecular or ionic dispersion of one substance in another. The particles in a solution are too small that they can’t be seen by the naked eye even with the aid of ultra microscope.
Solution
41
- do not have uniform composition
Heterogeneous mixture
42
- a mixture of whose particles are intermediate in size between a suspension and a solution. The particles can be seen through an ultra microscope
Colloid
43
– These are coarse mixtures, particles are visible with the naked eyes and settle out upon standing
Suspension
44
Properties of Matter
Physical and chemical properties
45
– those properties that may be received by the senses or measured by physical means.
Physical Properties
46
- those properties involved when matter undergoes chemical changes that is when a substance reacts with another substance.
Chemical Properties
47
Some chemical properties are:
1. Stability towards heat, light and pressure 2. Susceptibility to oxidation 3. Reactions with water or acid or other substances 4. Combustibility/Flammability 5. Stability 6. Relative Activity 7. Ionizations
48
properties do not depend on the size or amount of the sample. Colors, odor, boiling point, electrical conductivity are some examples
Intrinsic (intensive)
49
properties depend on the size or amount of the samples. Mass and volume are some examples.
Extrinsic (extensive)
50
– is one in which the substance is changed in appearance, state or properties but definitely not in composition.
PHYSICAL CHANGE
51
is the term applied to the change as solid turns into liquid
Melting
52
corresponds to the reverse process in which liquid turns into solid.
Freezing
53
are terms applied to the change as liquid turns into gas.
Evaporation and vaporization
54
corresponds to the reverse process in which gas turns into liquid
Condensation
55
is the term applied to the changes as solid turns directly into gas.
Sublimation
56
refers to the reverse process in which gas turns directly in a solid.
Crystallization
57
is one in which the appearance as well as the composition of the substances is changed resulting in one or more new substance/s. It is always accompanied by energy changes.
CHEMICAL CHANGE
58
Reactions that absorb energy are said to be ________
endothermic
59
those that release energy are _________.
exothermic
60
Electrolysis of water is an ________
endothermic reaction
61
burning is an _________
exothermic reaction.
62
– a molecular or ionic dispersion of one substance in another.
Solution
63
Physical properties example
1. Color. Silver and copper may be recognized by their color 2. Odor. Alcohol is easily differentiated from water by its odor. Hydrogen sulfide is easily detected because of its foul odor, similar to rotten egg. 3. Taste. Sugar is sweet, salt is salty 4. Solubility in water or other solvents. Sugar is very soluble in water while sand is insoluble in water. 5. Physical states. Matter can exist in three physical states namely solid, liquid and gas. 6. Density of Specific Gravity. Gases have low densities while solids have high densities. 7. Index of Refraction. Diamond is distinguished from ordinary glass because of its high refractive index. 8. Viscosity. Oil is more viscous than water 9. Colligative properties. Melting point, boiling point, freezing point, vapor pressure, osmotic pressure 10. Other properties like hardness, tensile strength, texture, electrical conductivity, shape, etc.
64
Physical properties example
Color Odor Taste Solubility in water Physical states Density Viscosity Colligative properties Other properties like conductibility, hardness, texture etc.
65
Carbon Dioxide, Carbides, Table Salts, Carbon Monoxide
Inorganic
66
Hydrogen, Oxygen, Nitrogen, Protein, Carbohydrates
Organic compound

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