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G12 [1st Sem] > [Prelim] Xy Chem > Flashcards

[Prelim] Xy Chem Flashcards

1
Q
  • Takes up space and has mass
  • Everything is made up of matter
  • Composed of tiny particles called atoms
  • Be in a form of solid, liquid, or gas
A

Matter

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2
Q
  • Consist even smaller subatomic particles
  • Such as: electrons, protons, and neutrons
A

Atom

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3
Q
  • Have a definite volume and maintain a definite shape
  • There is a strong force of attraction between particles and little free space
    between them, making these particles closely packed together and rigid
  • Tend to vibrate slowly and have fixed positions
A

Solids

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4
Q
  • Have a definite volume, but do not have a definite shape
  • Take the shape of the container
  • Not as closely held together as in solids
  • Liquid particles have more kinetic energy which is why they slide past each other.
A

liquids

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5
Q
  • Have no definite volume and no definite shape
  • Take the shape of their container
  • The force acting on the particles of gas is weak, which is why they tend to move
    past each other freely
  • Have high kinetic energy and have a lot of space between them, making the gas flow
A

Gas

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6
Q
  • Perceived by the senses
  • Can be measured and tested without changing the composition of matter
  • Ex. color, odor, taste, hardness, melting point, and boiling point
  • Extensive or Intensive
A

PHYSICAL PROPERTIES

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7
Q
  • properties that do not depend on the amount of matter present or being measured.
  • If the amount of matter is changed, the property will remain the same
  • Color, hardness, and boiling point are some examples of intensive properties
    (use the senses)
A

INTENSIVE PROPERTIES

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8
Q
  • properties that depend on the amount of matter present or being tested.
  • If there is a change in the amount of matter, these properties change, too.
  • Ex. volume, mass, length, and shape.
A

EXTENSIVE PROPERTIES

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9
Q
  • properties involved in the transformation of substances into other materials which possess a completely different structure and composition from the original.
  • Ex. flammability, reactivity, rusting (oxidation)
A

CHEMICAL PROPERTIES

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9
Q
  • the ability of matter to burn
A

FLAMMABILITY

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9
Q
  • the ability of matter to chemically combine with another.
A

REACTIVITY

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10
Q
  • a property of a material that pertains to the interaction on the surface of metals
A

Luster

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11
Q
  • the ability of a metal to be hammered or shaped into thin sheets without breaking of cracking.
A

MALLEABILITY

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12
Q
  • the ability of a metal to be drawn into thin wires
  • Metals are ductile because the atoms of metals can move past each other
    without breaking the metallic bond, which retains its structure
A

DUCTILITY

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13
Q
  • the tendency of a material to break even when a small amount of force is applied.
A

BRITTLENESS

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14
Q
  • the mass of an object per unit volume
A

Density

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15
Q
  • contains only one kind of element or compound
  • has a constant composition and cannot be separated by physical means
  • can be classified into elements and compounds.
A

PURE SUBSTANCES

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16
Q
  • substances composed only of only one kind of atom.
  • can be classified into metals, nonmetals, or metalloids
A

ELEMENTS

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17
Q
  • constitute the greatest number of elements in the periodic table
  • Lustrous, malleable & ductile, good conductors, solids, hard, and have high
    densities
A

METALS

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18
Q
  • lack the characteristics of metals
  • Dull in appearance, brittle, poor conductors of heat & electricity, and have low
    densities
A

NONMETALS

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19
Q
  • elements which have properties of both metals and nonmetals.
  • Ex. boron, germanium, antimony, and tellurium.
A

METALLOIDS

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20
Q
  • substances composed of two or more kinds of atoms that are chemically bonded together in fixed proportions.
  • Ex. acids, bases, and salts.
A

COMPOUNDS

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21
Q
  • made up of two or more substances which are mixed together but not chemically combined.
  • can be homogeneous or heterogeneous
  • Ex. Coffee, wine, air, brass, steal vinegar, blood, etc
A

MIXTURES

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22
Q
  • has only one phase and a uniform composition throughout.
  • difficult to distinguish the components of a homogeneous mixture
A

HOMOGENEOUS

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23
Q
  • has two or more phases.
  • Components of heterogeneous mixtures can be identified at times.
A

HETEROGENEOUS

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24
Q
  • Used for mixtures of insoluble solid in a liquid
  • Requires a filtering medium like cheesecloth or filter paper
  • Filter paper traps the insoluble solid while allowing liquid to pass through
  • This process is applicable for a mixture of sand in water
A

FILTRATION

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25
Q
  • The solid component that remained in the filtering medium
A

RESIDUE

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26
Q

The liquid collected

A

FILTRATE

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27
Q
  • Sedimentation allows heavier solid components to settle at the bottom.
  • Decantation is when heavier components are finally settled, the liquid above is
    poured into another container.
A

SEDIMENTATION AND DECANTATION

28
Q
  • If a mixture involves a substance that can easily transform from a solid state to its gaseous state
  • Ex. Mixture of naphthalene and salt. Slight increase of heat makes naphthalene sublime, leaving salt.
A

SUBLIMATION

29
Q
  • Used for mixtures of soluble solids in liquids, such as table salt in water
  • Water evaporates upon heating, leaving the salt crystals.
A

EVAPORATION

30
Q
  • Used for mixtures of two liquids with different boiling points through continuous evaporation and condensation processes
A

DISTILLATION

31
Q
  • Used to separate the components of inks
  • Using a mobile phase and stationary phase, the components rise in different
    speeds on the paper through capillary action
A

CHROMATOGRAPHY

32
Q
  • Proposed that everything is made of the four basic elements: fire, water, earth,
    and air
A

EMPEDOCLES (490-435 B.C)

33
Q
  • Known as the most influential Greek philosopher in his time
  • Aside from the four elements proposed by Empedocles, Aristotle added a fifth
    element, known as the Quintessence.
A

ARISTOTLE (384-323 B.C)

34
Q

Aside from the four elements proposed by Empedocles, Aristotle added a fifth
element, known as the ___________.

A

Quintessence

35
Q

Proposed that everything must be made of tiny and invisible particles which he
called “Atoms”

A

DEMOCRITUS (460-370 B.C)

36
Q

Democritus proposed that everything must be made of tiny and invisible particles which he
called “______”

A

Atoms

37
Q
  • In 1803, he proposed a concrete atomic theory
  • Proposed that atoms have fixed weights and definite properties
  • His theory led to the beginning of the modern era of Chemistry
A

JOHN DALTON

38
Q
  • In 1897, he discovered the presence of electrons in atoms using cathode rays
  • In 1900s, proposed his model of atom known as the plum-pudding model of an atom
A

JOSEPH JOHN THOMSON

39
Q
  • In 1909, he was able to determine the charge of an election, and its mass using the oil-drop experiment.
A

ROBERT ANDREWS MILLIKAN

40
Q

In 1900s, Joseph Thomson proposed his model of atom known as the _________ model of an atom

A

plum-pudding

41
Q

In 1909, Robert was able to determine the charge of an election, and its mass using the _______ experiment.

A

oil-drop

42
Q

In 1910, Ernes discovered the presence of protons in the nucleus of an atom, the positively charged particles using the famous ________ experiment

A

gold-foil

43
Q

In 1910, he discovered the presence of protons in the nucleus of an atom, the positively charged particles using the famous gold-foil experiment.

A

ERNES RUTHERFORD

44
Q
  • In 1932, he discovered another type of subatomic particle with no charge, the neutron
  • Added that neutrons can be found in the nucleus of an atom together with the protons
A

JAMES CHADWICK

45
Q

In 1913, proposed his atomic model known as Bohr’s model where the total energy of electrons is quantized, that is, restricted to having only specific values

A

NIELS BOHR

46
Q
  • Proposed by Antoine Lavoisier, who is also known as the father of modern Chemistry
  • States that the mass of the products in a chemical reaction will always be equal to the mass of the reactants
  • In other words; matter can neither be created nor be destroyed
A

LAW OF CONSERVATION OF MASS

47
Q
  • Published by Joseph Proust (french chemist)
  • States that different samples of the same compound always contain its constituent elements in the same proportion by mass
  • Ex. the water in the philippines and water in the U.S is the same
A

LAWS OF DEFINITE PROPORTIONS

48
Q
  • Published by John Dalton
  • States that if two elements can combine to form more than one compound, the
    masses of one element that can combine with a fixed mass of other element are in rations of small whole numbers.
A

LAW OF MULTIPLE PROPORTIONS

49
Q
  • The basic unit of matter
  • Consists of three main subatomic particles namely: protons, electrons, and neutrons
  • Contains a nucleus which is located at its center
A

Atom

50
Q
  • Small, negatively charged particles that spin around the nucleus, staying in orbits (shells or energy levels)
  • Shells are numbered, depending on how close they are to the nucleus
A

Electrons

51
Q
  • Positively-charged subatomic particle of an atom
  • Can be found in the nucleus, together with the neutron
A

PROTONS

52
Q
  • Are subatomic particles with no charge.
  • Like protons, neutrons are in the nucleus of an atom.
A

NEUTRONS

53
Q
  • equal to the number of protons inside the nucleus.
  • In a neutral atom, it is also equal to the number of electrons.
A

ATOMIC NUMBER (Z)

54
Q
  • the sum of the number of protons and neutrons in the nucleus
  • simply the approximation of the atomic mass since the mass of electrons is
    almost negligible
A

MASS NUMBER (A)

55
Q
  • atoms of the same element that have the same number of protons but different number of neutrons.
  • In other words, the isotopes of an element have the same atomic number but different mass number.
A

ISOTOPES

56
Q

used for detecting skin cancer

A

P-13

57
Q

used for medical diagnostic tests in thyroid glands

A

I-131

58
Q
  • is used in studying brain tumors.
A

Cu-64

59
Q
  • used for detecting blood clots and tumors
A

Na-24

60
Q

3 states of matter:

A

Solid
Liquid
Gas

61
Q

Physical Properties:

A

Intensive Properties
Extensive Properties

62
Q

Chemical Properties:

A

Flammability
Reactivity

63
Q

Classification of matter:

A

Pure substances
Elements
Compounds
Mixtures

64
Q

Elements:

A

Metals
Nonmetals
Metalloids

65
Q

Mixtures:

A

Homogeneous
Heterogeneous

66
Q

Methods of separating Mixtures:

A

-Filtration
-Sedimentation and Decantation
-Sublimation
-Evaporation
-Distillation
-Chromatography

67
Q

DEVELOPMENT OF THE MODERN ATOMIC THEORY

A

Empedocles
Aristotle
Democritus
John Dalton
Joseph John Thomson
Robert Andrews Millikan
Ernes Rutherford
James Chadwick
Niels Bohr

68
Q

3 basic laws of matter:

A

-law of conservation of mass
-laws of definite proportions
-law of multiple proportions

69
Q

Subatomic Particles:

A

Electrons
Protons
Neutrons

70
Q

Representing an atom:

A

Atomic number
Mass number
Isotopes
P-13
I-131
Cu-64
Na-24

G12 [1st Sem] (13 decks)

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