[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
2
Q
- Consist even smaller subatomic particles
- Such as: electrons, protons, and neutrons
A
Atom
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
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
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
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
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
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
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
9
Q
- the ability of matter to burn
A
FLAMMABILITY
9
Q
- the ability of matter to chemically combine with another.
A
REACTIVITY
10
Q
- a property of a material that pertains to the interaction on the surface of metals
A
Luster
11
Q
- the ability of a metal to be hammered or shaped into thin sheets without breaking of cracking.
A
MALLEABILITY
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
13
Q
- the tendency of a material to break even when a small amount of force is applied.
A
BRITTLENESS
14
Q
- the mass of an object per unit volume
A
Density
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
16
Q
- substances composed only of only one kind of atom.
- can be classified into metals, nonmetals, or metalloids
A
ELEMENTS
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
18
Q
- lack the characteristics of metals
- Dull in appearance, brittle, poor conductors of heat & electricity, and have low
densities
A
NONMETALS
19
Q
- elements which have properties of both metals and nonmetals.
- Ex. boron, germanium, antimony, and tellurium.
A
METALLOIDS
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
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
22
Q
- has only one phase and a uniform composition throughout.
- difficult to distinguish the components of a homogeneous mixture
A
HOMOGENEOUS
23
- has two or more phases.
- Components of heterogeneous mixtures can be identified at times.
HETEROGENEOUS
24
- 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
FILTRATION
25
- The solid component that remained in the filtering medium
RESIDUE
26
The liquid collected
FILTRATE
27
- 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.
SEDIMENTATION AND DECANTATION
28
- 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.
SUBLIMATION
29
- Used for mixtures of soluble solids in liquids, such as table salt in water
- Water evaporates upon heating, leaving the salt crystals.
EVAPORATION
30
- Used for mixtures of two liquids with different boiling points through continuous evaporation and condensation processes
DISTILLATION
31
- 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
CHROMATOGRAPHY
32
- Proposed that everything is made of the four basic elements: fire, water, earth,
and air
EMPEDOCLES (490-435 B.C)
33
- 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.
ARISTOTLE (384-323 B.C)
34
Aside from the four elements proposed by Empedocles, Aristotle added a fifth
element, known as the ___________.
Quintessence
35
Proposed that everything must be made of tiny and invisible particles which he
called “Atoms”
DEMOCRITUS (460-370 B.C)
36
Democritus proposed that everything must be made of tiny and invisible particles which he
called “______”
Atoms
37
- 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
JOHN DALTON
38
- 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
JOSEPH JOHN THOMSON
39
- In 1909, he was able to determine the charge of an election, and its mass using the oil-drop experiment.
ROBERT ANDREWS MILLIKAN
40
In 1900s, Joseph Thomson proposed his model of atom known as the _________ model of an atom
plum-pudding
41
In 1909, Robert was able to determine the charge of an election, and its mass using the _______ experiment.
oil-drop
42
In 1910, Ernes discovered the presence of protons in the nucleus of an atom, the positively charged particles using the famous ________ experiment
gold-foil
43
In 1910, he discovered the presence of protons in the nucleus of an atom, the positively charged particles using the famous gold-foil experiment.
ERNES RUTHERFORD
44
- 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
JAMES CHADWICK
45
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
NIELS BOHR
46
- 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
LAW OF CONSERVATION OF MASS
47
- 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
LAWS OF DEFINITE PROPORTIONS
48
- 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.
LAW OF MULTIPLE PROPORTIONS
49
- 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
Atom
50
- 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
Electrons
51
- Positively-charged subatomic particle of an atom
- Can be found in the nucleus, together with the neutron
PROTONS
52
- Are subatomic particles with no charge.
- Like protons, neutrons are in the nucleus of an atom.
NEUTRONS
53
- equal to the number of protons inside the nucleus.
- In a neutral atom, it is also equal to the number of electrons.
ATOMIC NUMBER (Z)
54
- 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
MASS NUMBER (A)
55
- 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.
ISOTOPES
56
used for detecting skin cancer
P-13
57
used for medical diagnostic tests in thyroid glands
I-131
58
- is used in studying brain tumors.
Cu-64
59
- used for detecting blood clots and tumors
Na-24
60
3 states of matter:
Solid
Liquid
Gas
61
Physical Properties:
Intensive Properties
Extensive Properties
62
Chemical Properties:
Flammability
Reactivity
63
Classification of matter:
Pure substances
Elements
Compounds
Mixtures
64
Elements:
Metals
Nonmetals
Metalloids
65
Mixtures:
Homogeneous
Heterogeneous
66
Methods of separating Mixtures:
-Filtration
-Sedimentation and Decantation
-Sublimation
-Evaporation
-Distillation
-Chromatography
67
DEVELOPMENT OF THE MODERN ATOMIC THEORY
Empedocles
Aristotle
Democritus
John Dalton
Joseph John Thomson
Robert Andrews Millikan
Ernes Rutherford
James Chadwick
Niels Bohr
68
3 basic laws of matter:
-law of conservation of mass
-laws of definite proportions
-law of multiple proportions
69
Subatomic Particles:
Electrons
Protons
Neutrons
70
Representing an atom:
Atomic number
Mass number
Isotopes
P-13
I-131
Cu-64
Na-24
