-classification -properties -phases

2.  anything that occupies space and has
mass.
 Macroscopic
 Microscopic
 Particulate

3.  Color of a liquid  Flammability of
alcohol
 Odor of a gas
 Density of gold
 Reactivity with HCl
 Melting point of sulfur
 Boiling point of water
 Volume of a metal
 Hardness of diamond sphere

4.  Can be determined without changing the
nature of the substance (color, odor,
physical state, density, hardness, melting
point and boiling point)

5.  Describes the ability of a substance to
participate in chemical reactions (reactivity
with oxygen, reactivity with acids,
flammability)

6.  Donot depend o the amount of the sample
being examined
 Depend on the quantity of the sample

7.  Odor  Hardness
 Color  Volume
 Weight  Area
 Mass  Thickness
 Density  Freezing point

12.  Has definite shape and definite volume
 Rigid
 Molecules are held tightly together
 Molecules can “wiggle” or vibrate only very
slightly

14.  Distinct
volume independent of its
container
 No specific shape
 Molecules slide over each other
 Pours easily

16.  No fixed volume or shape
 Moleculesare very far apart and are
moving at high speeds
 Moleculescolliding repeatedly with each
other and with the walls of the container

19. Copper

20. Nitrogen

21.  Highly ionized state
 positively charged ions

 Free negatively charged electrons
 99% of the matter in the universe

22. BOSE-EINSTEIN CONDENSATE (BEC)
 Predicted in 1924 by Albert Einstein, who
built on the work of Styendra Bose
 Condensation occurs when individual
atoms meld into a “superatom” behaving
as a single entity at just a few hundred
billionths of a degree above absolute zero

25. Chemical Initial state Final state Physical or
System Chemical
Change?

26. PHYSICAL Change
 Changes that alter the physical form of
matter without changing its chemical
identity.
 ALL changes of state are physical changes

27. CHEMICAL Change
 Occurswhen the chemical identity of a
substance is destroyed and a new
substance is formed.
 Chemical reactions

28. Indicators of Chemical change/reaction
 Color changes
 Odor changes
 Production of gas
 Production of solid or precipitate

29. Physical and Chemical Changes and Properties
Chemical Physical
Changes Old substances New form of old
destroyed substance
New substances No new substance
formed formed
Properties Properties defined Description by
by types of senses
chemical changes
possible Measurable
properties

30. ENDOTHERMIC Process
 The system absorbs heat
SURROUNDINGS HEAT
SYSTEM
 Melting of ice

31. EXOTHERMIC Process
 The system evolves heat
SYSTEM HEAT
SURROUNDINGS

32.  Combustion
 Freezing of water
 Melting of ice
 Boiling of water
 Condensing steam

34.  Has its own set of chemical and physical
properties
 Cannot be separated into parts by physical
means
 Has a definite, fixed composition that does
not vary from one sample to another

35.  Consists of two or more chemicals
 Properties depend on the substances on it
 Compositions can vary

36.  Definedby its atomic number
 Cannot be decomposed into simpler
substances
Atomic Number - the number
of protons in an unreacted
atom
Mass Number - the number of
protons and neutrons together

38. Hydrogen H 63.0%
Oxygen O 25.5%
Carbon C 9.45%
Nitrogen N 1.35%
Calcium Ca
Phosphorus P
Chlorine Cl
Sulfur S 0.7%
Sodium Na
Potassium K
Magnesium Mg

39. a substance made of more than one type
of atom
 Composed of 2 or more elements
 Atoms combined in fixed proportions
 Can be decomposed into two or more
other substances by chemical change

40.  Turnblue litmus to red
 React with many metals
 React with bases

41.  An acid can be defined as a substance
that yields hydrogen ions (H+) when
dissolved in water.
 HCl
• Pure substance, hydrogen chloride
• Dissolved in water (H+ Cl-), hydrochloric acid
 Anoxoacid is an acid that contains
hydrogen, oxygen, and another element.

42.  Cause color changes in plant dyes.
 React with certain metals to produce
hydrogen gas.
2HCl (aq) + Mg (s) MgCl2 (aq) + H2 (g)
 Reactwith carbonates and bicarbonates to
produce carbon dioxide gas
2HCl (aq) + CaCO3 (s) CaCl2 (aq) + CO2 (g) + H2O (l)
 Aqueous acid solutions conduct electricity.

43.  pH – A Measure of Acidity

46.  Turnred litmus to blue
 React with acids

47. A base can be defined as a substance that
yields hydroxide ions (OH-) when dissolved
in water.
NaOH sodium hydroxide
KOH potassium hydroxide
Ba(OH)2 barium hydroxide

48.  A salt, is defined as the product formed
from the neutralization reaction of acids
and bases. Salts are ionic compounds
composed of cations (positively charged
ions) and anions (negative ions) so that
the product is electrically neutral (without a
net charge)

49. acid + base salt + water
HCl (aq) + NaOH (aq) NaCl (aq) + H2O
H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O
H+ + OH- H2O
4.3

51. Wala akong boses
Kaya please, konting katahimikan at pag-
itindi ang aking hiling 
Salamat,
Ma’am Pie 

52. 1. Identify the physical state of the following:
a) Helium in a toy balloon
b) vitamin tablets in a bottle
c) mercury in a thermometer

53. 2. Identify the type of property in the
following statements:
a. Yellow-green chlorine gas attacks silvery
sodium metal to form white crystals of
sodium chloride.
b. A magnet separates the mixture of black
iron shavings and white sand.

54. 3. State which type of change occurs in the
following statements:
a. Passing an electric current through
molten magnesium chloride yields molten
magnesium and gaseous chlorine.
b. The iron in discarded automobiles forms
reddish brown, crumbly rust.

55. c. Chopping a log
d. Burning a log
e. Toasting a slice of bread

56. 4. What is the key difference between an
element and a compound?
5. List two differences between a compound
and a mixture.
6. Make a concept of the Classification of
Matter.

57. HETEROGENEOUS
 Varies in composition and or properties
from one part of the mixture to another
HOMOGENEOUS
 Has the same/uniform composition and
properties throughout

59. Kind of mixture Particle size Examples Characteristics

60. SUSPENSION
 >1000 nm
 Particles are more or
less evenly dispersed
throughout a liquid or
gas
 Different parts
separate over time

62. SOLUTION
 0.2-2.0 nm
 A homogeneous mixture of two or more
substances uniformly dispersed throughout
a single phase

63. Gas Liquid Solid
Gas Oxygen and The odor of a
other gases in Water vapor in solid --
nitrogen (air) air (humidity) molecules of
that solid being
dissolved in the
air
Liquid Carbon dioxide Ethanol Sucrose (table
in water (common sugar) in water;
(carbonated alcohol) in sodium chloride
water) water; various (table salt) in
hydrocarbons in water
each other
(petroleum) *
Solid Hydrogen Water in Steel, Brass,
dissolved to activated other metal
palladium charcoal alloys

64. COLLOID
 2.0-1000 nm
 Consists of tiny particles that are
suspended in a liquid, solid, or gas
 Stable heterogeneous mixtures
 Exhibits Tyndall effect

66.  Decantation
• separates liquids from solids that have settled
 Evaporation
• Separates the solid (residue) from the liquid
(filtrate) parts of the mixture

67.  Distillation

68.  Filtration

69.  Centrifugation

70.  Chromatography

72.  Sugar dissolved in water
 Mixture of ethyl alcohol and water
 Mixture of salt and sand
 Iron filings, mongo seeds and salt mixture