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Measurement
Quantative observation with a value number and a unit
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Scientific Notation
standard way of expressing large as well as small numbers
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Significant Figures
(digits) (sf) reflects precision of a given number
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Exact number
Number with unlimited (Sf)
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Unit
standard agreed upon quantities by which measurements are made
(eng & metric unit) (Scientist us SI units)
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Metric system
uses prefixes multipliers to change the magnitude the size of units
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Length
is a measure of distance between two points- measured with a ruler
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Volume
is a measure of a 3dimensional space occupied by an object
measured using graduated cylinder
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Mass
is a measure of quantity of material (matter)
measured with balance
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Weight
is a measure of force of gravity acting upon an object
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Unit conversion
changing from one unit to another for particular measurements
using conversion factors derived form equivalents
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Density
is a measure of a mass per volume
the ratio of mass to volume
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Matter
is anything which has mass and occupies space
consists of small particles like atom + molecules
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Energy
is the ability to do work
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Atom
is the smallest indivisible particle of any matter
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Molecule
is a smaller particle with groups of atoms bond together
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Element
is a substance which consists of same kind of atoms.
(homoatomic)
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Compound
is a substance which consists of more than one kind of atoms bounded together
- (heteroatomic)
- matter, molecule, element & compound
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Chemistry
is a branch of science which studies matter to the molecular level
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Scientific method
systematic way of learning through experiment and observation
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Hypothesis
- is a tenative explanation based on observation
- (can be modified)
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Scientific theory
- is a well established hypothesis
- (can be modified with time)
which provides broader and deeper explanation based on many similar observations
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Atomic theory
Atom is the smallest indivisible particle (small unit) of any matter
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Scientific Law
statements given based on many similar observation with no exceptions to the rule
(can not be modified with time)
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Law of conservation
Matter can neither be created nor destroyed.
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Solid
- Particles that have definite (fixed) shape + volume
- Incompressible
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Liquid
Particles that have no fixed shape but have fixed volume
Incompressible
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Gas
particles that do not have definite shape of volume
Highly compressible
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Pure substance
is a substance of consisting of same type of particles
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Element
is a pure substance consisting of same type of atoms, which can not be broken down to simpler substances
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Compound
is a pure substance consisting of particles, which is a chemical combination of two or more elements in a fixed ratio
can be broken down to simpler substance
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Mixture
is a physical combination of two or more substances with no fixed ratio
Consists of more than one type of particle (atom + molecules)
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Hemogeneous Mixture
uniform mixture of two or more substances whose composition is same through all different regions
Air, Alloys, soda, sea water, alcoholic drinks
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Heterogeneous Mixture
Non uniforms mixture of two or more substances, whose composition is not same through different regions.
Milk, blood, oil + water, sand + water, paint
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Physical properties
are characteristics exhibited with no change in composition (no new particles formed)
viscosity, boiling point, freezing point
Reversible
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Chemical properties
are characteristics exhibited with a change in composition - New particles formed
acidity, toxicity, flammability, corrosiveness
irreversible
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Mixture of insoluble solid + liquid
Heterogeneous Mixture
sand + water
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Mixture of soluble solid + water
Homogeneous Mixture
sodium chloride + water
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Mixture of two liquids which are miscible (mixed very well)
Homogeneous Mixture
Alcohol + water
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Mixture of two liquids which are immiscible (do not mix)
Heterogeneous Mixture
oil + water
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Energy
is ability to work
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Law of conservation of energy
Energy can neither be created or destroyed
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Potential energy
is the stored form of energy
is the energy of particle at rest
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Kinetic Energy
is the energy of a moving particle
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calorie
is the amount of energy required by one gram of water to change by 1 degree celcius
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Temperature
is a measure of intensity of heat
measurement related to the relative movement of particles
measured using a thermometer
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Specific heat capacity
is the amount of energy required by one gram of a substance to change by 1 degree celcius
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Heat
is the thermal energy exchanged due to temperature differences
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Exothermic
energy released, given out, lost, is a product
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Endothermic
energy absorbed, gained, taken in is a reactant
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Atom:
is the smallest particle (single unit) of any matter
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Electrons
are lighter negatively charged particle found within an atom
Symbol e1-
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Protons
are heavier positively charged particles found in the heavy center core of the atom called the nucleus
symbol p1+
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Neutrons
are as heavy as a proton
symbol n0
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Subatomic particles
particles found within an atom
what are they, scientist, exp, model/theory, symbol, relative charge, relative mass, location
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Atomic number
stands for the number of protons
# of electron
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Mass number
stands for the total number of protons + neutrons
dont mistake with atomic mass
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amu- atomic mass unit
is equal to 1/12th the mass of carbon-12 which has 6 protons and 6 neutrons
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Isotopes
are atoms of the same element with different mass number
are atoms of the same element with different number of neutrons
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Atomic mass of an element
is the average relative isotopic mass of all the isotopes of a given element
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Isotopic abundance
is the extent to which an isotope is available in nature
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Natural abundance
all isotopes are not present to the same extent
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Symbols of elements
are with one or two letters derived form english, latin or greek names of elements
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Mendeleev
Father of periodic table
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Periodic law
when elements arranged by increasing relative atomic mass sets of properties of elements recur periodically
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Modern Periodic table
elements are arranged by increasing atomic number
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Ions
are charged particles formed by the loss or gain of electrons
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Positvie ion
Cation-is formed by the loss of electron by metallic element
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Negative ion
is formed by the gain of the electrons by non metallic elements
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Noble gas Rule
Main group elements tend to lose or gain electrons to become stable like nearest noble gas
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