Studied by 10 people
Density
mass/volume; in intensive (does not depend on the amount of material present)
What is an intensive property?
does not depend on the amount of material present
what is an extensive property?
does depend on the amount of material present
The Particulate Nature of Matter
all nature is made up of matter. More specifically, everything we see is comprised of the ~ 100 elements on the Periodic Table, which are made up of atoms
What can matter be divided into?
pure substances and mixtures
Elements
appear on the periodic table, and are made up of only one type of atom, with characteristics specific to that particular type of element
Compounds
made up of two or more atoms joined together in specific ratios by chemical bonds. Because they are joined by chemical bonds, they are considered to be pure substances even though they may have more than 2 types of elements
Mr. BrINCHlHOF
Br;I;N;Cl:H;O;F (put in calculator before test)
What is a solid (state of matter)
fixed volume and fixed shape
What two categories can solids be put into
Amorphous (no long-range structural pattern) or crystalline (meaning that they have long-range order)
Liquid (state of matter)
fixed volume but no fixed shape
Gas (state of matter)
no fixed volume or shape
What is an allotrope?
one of two or more different form in which an element can exist. For example diamond and graphite are 2 allotropes of the pure element carbon
physical properties
Can be observed or measured without changing the chemical composition of the material being described. Mass, color, boiling point, and density are examples of physical property
chemical properties
properties that relate to the ability to form new substances. these properties can routinely be observed without changing the composition of the material. Combustibility, acidity reactivity, and toxicity are examples
Physical Changes
changes in state, such as boiling, melting, sublimating, condensing, or freezing. Breaking an object, mixing two or more substances together. All the chemical composition of the material is not affected.
Chemical Changes
involve a change to the chemical composition of the material in question. Combustion and rusting are examples of chemical changes. (color changing is a chemical change)
homogeneous mixtures
even distribution; carbonated beverage or cup of coffee
heterogeneous mixture
not evenly distributed; soil or soup are examples
alloy
a mixture of elements that has metallic properties
substutional alloy
comprised of two or more metals, wherein minority component atoms replace some atoms of the major component
interstitial alloy
comprised of a metal and non-metal, in which the non-metal atom fits within the intersects (holes) between metal atoms
Antonie Lavoisier
law of conservation of mass
Joseph Proust
law of definite proportions
John Dalton
law of multiple proportions; early atom model
J.J. Tompson
discovered the electron; plum pudding model
Robert Millikan
discovered charge and mass of electron
Earnest Rutherford
discovery of nucleus and protons
James Chadwick
discovered neutrons
Dmitri Mandeleev
organized the periodic table
Niels Bohr
planetary model of the atom
Louis de Broglie
the wave model of the atom
Erwin Schrodinger
the quantum model of the atom
atomic structure
positive protons and un-charged neutrons in the nucleus, negatively charged electrons orbiting, mass of neutron and protons nearly identical.
isotopes
Atoms of the same element that have different numbers of neutrons
alkali metal
any metal in Group 1A of the periodic table
anion
A negatively charged ion
binary molecule
A molecule composed of exactly two different elements.
electron
negatively charged particle
ionic compounds
compounds composed of cations and anions
metals
Elements that are good conductors of electric current and heat.
neutrons
the particles of the nucleus that have no charge
polyatomic ion
A charged group of covalently bonded atoms
alkaline earth metal
An element in Group 2A of the periodic table; a very reactive metal having an oxidation number of +2.
atomic number (z)
the number of protons in the nucleus of an atom
cation
A positively charged ion
halogen
a nonmetal in Group 7A of the periodic table - 1
isotope
Atoms of the same element that have different numbers of neutrons
metaloids
(semiconductors) are the elements that have the properties of both metals and nonmetals
noble gases
the elements in Group 8A of the periodic table no charge
proton
positively charged particle
allotropes
Different forms of the same element
binary acid
an acid that contains only two different elements: hydrogen and one of the more electronegative elements
Electrolyte
A substance that dissolves in water to give a solution that conducts electric current
ion
A charged atom
mass number (A)
the sum of the number of neutrons and protons in an atomic nucleus
molecular compounds
A compound consisting of molecules of covalently bonded atoms
non-metals
an element or substance that is not a metal.
Transitional Metals
elements in groups 3-12
know how to do isotope and ion table
(z and p are the same number) (A is the periodic table number) (N = A - P) #e- is n with the inverted charge for example (charge is -3 and N is 20 #e- is 23)
Know the atomic mass problem
%/100 x The element number
the symbol of frequecy
v
symbol of wavelength
λ
symbol of
c
Planck's constant
6.626 x 10^-34 (h)
principle quantam number
(n >= 1)
angular momentup quantam number
(l = 0 to (n-1))
magnetic quantum number
m sub l = -l to l
spin quantam number
denotes which electron in the orbital you're talking about; only 2 per orbital; one spins up and one spins down
use program for electron config on calculator
.
l = 0 - s - 1 - 2
.
l = 1 - p - 3 - 6
.
l = 2 - d - 5 -10
.
l = 3 - 4 - 7 - 14
.
bond length
the average distance between the nuclei of two bonded atoms
bond strength
energy required to break a bond
covalent bonding radius
a measure of the size of an atom that forms part of one covalent bond
effective nuclear charge (Zeff)
amount of charge felt by the most recently added electron
electorn affinity
how much an atom wants to gain an electron
Electronegativity
A measure of the ability of an atom in a chemical compound to attract electrons
electron shielding
the reduction of the attractive force between a positively charged nucleus and its outermost electrons due to the cancellation of some of the positive charge by the negative charges of the inner electrons
ionic bonds
Formed when one or more electrons are transferred from one atom to another
ionization energy
The amount of energy required to remove an electron from an atom
Isoelectronic
having the same number of electrons
lewis dot structures
diagrams that show valence electrons as dots
metallic characters
metals, metalloids, nonmetals
Non-bonding pairs
two paired valence electrons that tend not to participate in a chemical bond
octet rule
States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons
valence shell electrons
electrons in the outermost shell
van der Waals forces
a slight attraction that develops between the oppositely charged regions of nearby molecules
be able to explain the periodic trends
see review
be able to show lewis dot structure with elements
(no compounds)
the three kinds of chemical bonds
ionic, covalent, metallic
formula unit
the smallest electrically neutral collection of ions
acids have what as the first element
hydrogen (exceptions are H2O and H2O2
what does mono, di, tri, and tetra mean
1, 2, 3, 4
ammonium
NH4+
Cabonate
CO3 2-
Hydride
OH-1
Nitrate
NO3 -1
Note 
Flashcard (37)