Chemistry Final
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116 Terms
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chemistry
The study of the properties of matter and how matter changes
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scientific method
a procedure to understand information
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measurement
a quantity that has both a number and a unit
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theory
A hypothesis that has been tested with a significant amount of data
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natural law
rules of conduct discoverable by reason
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model
A representation of an object or event
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hypothesis
A testable prediction
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prediction
A statement of what will happen next in a sequence of events
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experiment
a set of controlled observations that test the hypothesis
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quantitative data
numerical data
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qualitative data
descriptive data
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scientific notation
A mathematical method of writing numbers using powers of ten
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unit
A standard quantity in terms of which other quantities may be expressed.
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metric system
a system of measurement based on the number 10
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english system
a system of measuring that uses length units of inches, feet, and miles
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SI units
The preferred metric units for use in science
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volume
The amount of space an object takes up
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mass
the amount of matter in an object
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significant figures
All the digits that can be known precisely in a measurement, plus a last estimated digit
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rounding off
A procedure used for deleting nonsignificant figures
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conversion factor
a ratio of equivalent measurements
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equivalence statement
a statement that relates different units of measurement
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dimensional analysis
A way to analyze and solve problems using the units, or dimensions, of the measurements
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milliliter
mL (1/1000)
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metric prefixes
kilo, hecto, deca, deci, centi, milli, nano, macro
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liter
Basic unit of volume in the metric system
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Celcius scale
The temperature scale on which zero and 100 are the temperatures at which water freezes and boils
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Farhenheit Scale
the termperature scale on which 32 and 212 are the freezing and boiling point of water
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Kelvin Scale
The temperature scale on which zero is the temperature at which no more energy can be removed from matter
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accuracy
how close a measurement is to the true value
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precision
a measure of how close a series of measurements are to one another
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density
mass/volume
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matter
anything that takes up space and has mass
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atoms
smallest unit of matter
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elements
any substance that cannot be broken down into simpler substances
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compounds
molecules that contain more than one element
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molecules
two or more atoms joined together
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alloy
A mixture of two or more metals
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solution
A mixture that forms when one substance dissolves another.
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homogeneous mixture
A mixture in which substances are evenly distributed throughout the mixture
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heterogeneous mixture
A mixture in which different materials can be distinguished easily
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physical properties
the characteristics of a substance that can be observed or measured without changing the substance
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chemical properties
Characteristic that cannot be observed without altering the substance
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physical change
A change in a substance that does not change its identity
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chemical change
A change in matter that produces one or more new substances
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solid
Definite shape and volume
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liquid
definite volume but no definite shape
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gas
no definite shape or volume
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electrons
Negatively charged particles
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protons
Positively charged particles
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neutrons
the particles of the nucleus that have no charge
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nucleus
center of an atom made of protons and neutrons
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element
A pure substance made of only one kind of atom
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istopes
Atoms of the same element that have different numbers of neutrons
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atomic number
number of protons
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mass number
the sum of the number of neutrons and protons in an atomic nucleus
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Dalton's Law
at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases
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conversation of mass
matter cannot be created or destroyed
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metals
good conductors of heat and electric current
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nonmetals
poor conductors of heat and electric current
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metalloids
Elements that have properties of both metals and nonmetals.
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Periodic Table
A chart of the elements showing the repeating pattern of their properties
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groups
Vertical columns on the periodic table
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periods
Horizontal rows on the periodic table
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atomic size
size of an atom
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alkali metals
Group 1
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alkaline earth metals
Group 2
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halogens
Group 3
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noble gases
Group 18
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diatomic molecules
H2, N2, O2, F2, Cl2, Br2, I2 (Have NO Fear Cold Beer On Ice
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allotropes
Different forms of the same element
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ionic compounds
compounds composed of cations and anions
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ions
positively and negatively charged atoms
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cations
positively charged ions
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anions
negatively charged ions
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ionization energy
The amount of energy required to remove an electron from an atom
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electronegativity
the ability of an atom to attract electrons when the atom is in a compound
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chemical formula
shows the elements in the compound and the ratio of atoms
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binary compounds
compounds composed of two elements
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type I metals
Group 1a Group 2a Al, Ga, Zn, Ag NH4+
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type II cations
group B elements and atoms under the staircaise (Not including aluminum)
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ionic bonds
nonmetals and metals
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covalent bonds
nonmetals with nonmetals
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polyatomic ions
ions that are made of more than one atom
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hydro acids
Hydro + halogen name + ic
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oxy acids
contains hydrogen, oxygen, and 1 other element (polyatomic ions)
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acid
any compound that forms H+ ions in solution
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base
A substance that decreases the hydrogen ion concentration in a solution.
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dissolve
to form a solution by mixing evenly
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dissociate
to separate
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strong electrotype
conducts an electric current when dissolved in water
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weak electrotype
separates into different cations and anions when dissolved in water
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nonelectrolyte
a liquid or solid substance or mixture that does not allow an electric current
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Avogadro's number
6.02 x 10^23
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one mole
6.02 x 10^23 representative particles of a substance
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reactants
A starting material in a chemical reaction
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products
The elements or compounds produced by a chemical reaction.
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converting from C to K / K to C
C + 273 = K / K - 273 = C
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multiplication/division
least number of sig figs
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addition/subtraction
least number of decimal places
Note 
Flashcards (78)