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SELF-STUDY > Part 2 Science > Flashcards

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
Q

Have definite composition

A

Compound

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26
Q

Have variable composition

A

Mixture

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27
Q

Always homogeneous

A

Compound

28
Q

Maybe homogeneous or heterogeneous

A

Mixtures

29
Q

Have definite properties

A

Compound

30
Q

Have variable properties depending on
the amount of components

A

Mixtures

31
Q

The constituents are chemically combined

A

Compound

32
Q

The components are not chemically
combined

A

Mixtures

33
Q

The constituents may be separated
only by chemical means

A

Compound

34
Q

the components may be separated by
physical or chemical means

A

Mixtures

35
Q

Constituents are the particles that composed a _______

A

compound

36
Q

Components are the particles that composed a _______

A

mixture

37
Q

composed of two or more substances in a variable composition

A

Impure substance or mixtures

38
Q

Mixtures are classified into:

A

Homogeneous
Heterogeneous

39
Q
  • composed of uniform composition and made up of only one phase
A

Homogeneous mixture

40
Q

– 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.

A

Solution

41
Q
  • do not have uniform composition
A

Heterogeneous mixture

42
Q
  • a mixture of whose particles are intermediate in size between a suspension and a
    solution. The particles can be seen through an ultra microscope
A

Colloid

43
Q

– These are coarse mixtures, particles are visible with the naked eyes and settle
out upon standing

A

Suspension

44
Q

Properties of Matter

A

Physical and chemical properties

45
Q

– those properties that may be received by the senses or measured by
physical means.

A

Physical Properties

46
Q
  • those properties involved when matter undergoes chemical changes
    that is when a substance reacts with another substance.
A

Chemical Properties

47
Q

Some chemical properties are:

A
  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
Q

properties do not depend on the size or amount of the sample. Colors, odor, boiling
point, electrical conductivity are some examples

A

Intrinsic (intensive)

49
Q

properties depend on the size or amount of the samples. Mass and volume are some
examples.

A

Extrinsic (extensive)

50
Q

– is one in which the substance is changed in appearance, state or
properties but definitely not in composition.

A

PHYSICAL CHANGE

51
Q

is the term applied to the change as solid turns into liquid

A

Melting

52
Q

corresponds to the
reverse process in which liquid turns into solid.

A

Freezing

53
Q

are terms applied to the change as liquid turns into gas.

A

Evaporation and vaporization

54
Q

corresponds to the reverse process in which gas turns into liquid

A

Condensation

55
Q

is the term applied to the changes as solid turns directly into gas.

A

Sublimation

56
Q

refers to the reverse process in which gas turns directly in a solid.

A

Crystallization

57
Q

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.

A

CHEMICAL CHANGE

58
Q

Reactions that absorb energy are said to be ________

A

endothermic

59
Q

those that
release energy are _________.

A

exothermic

60
Q

Electrolysis of water is an ________

A

endothermic reaction

61
Q

burning is an _________

A

exothermic reaction.

62
Q

– a molecular or ionic dispersion of one substance in another.

A

Solution

63
Q

Physical properties example

A
  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
Q

Physical properties example

A

Color
Odor
Taste
Solubility in water
Physical states
Density
Viscosity
Colligative properties
Other properties like conductibility, hardness, texture etc.

65
Q

Carbon Dioxide, Carbides, Table Salts, Carbon Monoxide

A

Inorganic

66
Q

Hydrogen, Oxygen, Nitrogen, Protein, Carbohydrates

A

Organic compound

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