Ch1-2 Flashcards
experiment
observation of natural phenomena carried out in a controlled manner
law
observations in nature that are repeated and give the same result
mass
the quantity of matter in a material
weight
the force of gravity exerted on an object
matter
whatever occupies space and can be perceived by our senses
law of conservation of mass
Lavoisier stated that total mass remains constant during a chemical reaction
fixed shape/fixed volume/neither
1) solid
2) liquid
3) gas
1) fixed shape, fixed volume
2) no fixed shape, fixed volume
3) no fixed shape, no fixed volume
1) physical change
vs
2) chemical change
1) change in the form of matter but not in its chemical identity
2) change in which one or more kinds of matter are transformed into a new kind of matter
distillation
process of separating an easily vaporized liquid from another substance (water from sodium chloride)
1) physical property
vs
2) chemical property
1) characteristic that can be observed without changing chemical identity
(color)
2) a characteristic involving its chemical change
(chemical property of iron = rust)
mixtures are separated by a ____ property
physical
elements in a compound are separated by a ____ property
chemical
1) substance
vs
2) element
1) kind of matter that cannot be separated into other matter by physical processes (EX: sodium chloride only separated by chemical)
2) a substance that cannot be decomposed by any chemical processes into simpler substances
(EX: arsenic, mercury, etc)
1) compound
vs
2) mixture
1) a substance composed of two or more elements chemically combined; can be separated
(water = hydrogen + oxygen)
2) the combination of two or more substances in which substances retain their distinct properties
(dissolving salt in water, can be distilled)
1) law of definite proportions
vs
2) law of multiple proportions
1) a pure compound always contains constant proportions of the elements by mass
2) when two elements form more than one compound, the masses of one element have a fixed ratio for the mass of the other element
(ex: CO 2:1 mass, CO2 2:1 mass)
a solution is also known as
a homogeneous mixture
602200 in scientific notation
6.022 x 10^5
.000166 in scientific notation
1.66 x 10^-4
precision vs accuracy
precision = closeness of a set of values to one another
accuracy = closeness of a single measurement to correct value
350 + 93,000,000 in sig figs
93,000,000 because since 100,000 is next biggest column and 350 doesn’t fit there, it is not added on
measured number vs exact number
1) measured = number which is observed and recorded in an experiment
2) recorded= number that arises when you count items (9 coins)
prefixes
kilo (10^3) hecto (10^2) deca (10^1) UNIT deci (10^-1) centi (10^-2) milli (10^-3) micro (10^-6) nano (10^-9)
1 mL =
1 m^3
atomic theory
an explanation of the structure of matter
4 main points of dalton’s atomic theory
1) elements are composed of extremely small particles called atoms
2) atoms of a given element are identical, having the same size, mass, and chemical properties
3) compounds are composed of atoms of more than one element (equal ratio)
4) a reaction only involves the separation, combination or rearrangement of atoms
atom-
an extremely small particle of matter
chemical reaction-
the rearrangement of atoms present in the reactants
nucleus-
the atom’s central core, positively charged
what did each person discover?
1) chadwick
2) rutherford
3) thomson
4) dalton
1) neutrons
2) nucleus
3) electrons
4) atom
atomic number
number of protons
mass number
total number of protons and neutrons
isotopes
atoms whose nuclei have same atomic number but different mass numbers (neutron numbers)
how does dalton use the laws of chemical composition in his atomic theory?
1) elements are composed of the same atom = law of definite proportions
2) a reaction only involves the separation, combination or rearrangement of atoms = law of conservation of mass
what points in john dalton’s atomic theory are still considered valid as he presented them?
atoms are the smallest particles
describe ONE discovery that changed the view of the atom and how it changed the atomic view
not all elements are identical = isotopes
fractional abundance
the fraction of the total number of atoms that is composed of an isotope
an atom that is most abundant is ____
the closest to its average atomic mass
period vs group
period = horizontal
group = vertical
metal vs nonmetal vs metalloid
1) metal = solids at room temp
2) nonmetal = gases/solids at room temp
3) metalloid = has both metallic and nonmetallic properties
1) molecular formula
vs
2) structural formula
1) gives the exact number of different atoms of an element in a molecule (H2O)
2) shows how the atoms are bonded together in a molecule (H-O-H)
molecule-
definite group of atoms chemically bonded together by attractive forces
polymers
vs
monomers
large polymers are made of smaller monomers
ion
an electrically charged particle obtained from an atom or chemically bonded group of atoms by adding or removing atoms
anion vs cation
1) anion- negatively charged ion, when an atom gains an electron
2) cation- positively charged ion, when an atom loses an electron
monatomic ion
vs
polyatomic ion
1) single atom ion (H+)
2) ions made up of more than one atom (NO2-)
ionic compounds
vs
molecular compounds
1) between two metals (transfer electrons)
2) between two or more nonmetals (share electrons)
differentiate between an isotope’s atomic mass and an element’s average atomic mass (atomic weight)
1) atomic mass is total number of protons and neutrons
2) average atomic mass is the sum of all of the isotopes masses and their fractional abundance’s
organic compounds
molecular substances that contain carbon combined with other elements (H, O, N)
hydrocarbons
compounds containing only hydrogen carbon (CH4 methane)
functional group
a reactive portion of a molecule that undergoes predictable reactions
chemical nomenclature
the systemic naming of chemical compounds
inorganic compounds
compounds composed of elements other than carbon
chemical equation
the symbolic representation of a chemical reaction in terms of chemical formulas
pure water is an example of a
compound
since the sample of salt and water tastes the same from the top and bottom of the container it is an example of a
homogenous mixture
it is cold when it is 32 degrees outside
false
a measurement is a number
false
the formula of the ionic compound formed by (Na, Group IA) and oxygen (O, Group VIA) is
Na2O
