exam 2 Flashcards
arranged elements by atomic mass
Newlands
discovered correlation between the number of protons and the frequency of x-rays generated
Moseley
groups 1A to 7A
main group elements
group 8A; have completely filled p subshells
noble gases
group 1B and 3B to 8B
transition metals
make up the f-block transition elements
lathanides and actinides
outermost electrons of an atom
valence electrons
independently proposed the idea of periodicity
Mendeleev and Meyer
3 things valence electrons are responsible for
- formation of chemical bonds
- help predict chemical properties
- usually the only electrons that interact with other atoms to form chem. bonds
actual magnitude of positive charge that is experienced by an electron in the atom
effective nuclear charge
where an electron is partially blocked from the positive charge of the nucleus by other electrons
sheilding
Zeff increases from..
left to right
distance between the nucleus of an atom and its valence shell
atomic radius
atomic radius in metals
metallic radius
atomic radius in nonmetals
covalent radius
atomic radius increases…
top to bottom; right to left
relative ability of an atom to attract a bonding pair of electrons affected by atomic radius; can only be measured for one element relative to another
electronegativity
has the highest electronegativity
Fluorine
minimum energy required to remove an electron from an atom in the gas phase
ionization energy
ionization energy increases..
left to right, bottom to top
energy released when an atom in the gas phase accepts an electron
electron affinity
electron affinity increases…
left to right, bottom to top
shiny, lustrous, malleable, ductile, good conductors, low ionization energies
metals
not shiny, brittle, poor conductors, high electron affinities
nonmetals
species with identical electron configurations to the noble gas to the right
isoelectric
radius of a cation or anion
ionic radius
When an atom loses an electron the radius…
decreases
when an atom gains an electron the radius…
increases
series of two or more species that have identical e- configurations but different nuclear charges
isoelectronic series
substance composed of two or more elements combined in a specific ratio and held together by chemical bonds
compounds
suggested that atoms combine to achieve a more stable electron configuration
Lewis
method used for depicting the valence electrons of the atoms involved in a compound
lewis dot symbols
elements with low ionization energies tend to form…
cations
elements with high ionization energies tend to form…
anions
when cations and anions are brought together
ionic compounds
most common ionic compounds
binary compounds
typically hold ionic compounds together
ionic bonds
3-D array of anions and cations
lattice
energy change associated with the formation on ionic bonds
lattice energy
the greater the lattice energy ( ) stable the compound
MORE
if the distance between two elements in an ionic bond increases, the lattice energy will….
decrease
consists of a single atom with more or less electrons than protons
monatomic ions
combination of at least two atoms in a specific arrangement held together by chemical forces
molecule
different samples of a given compound always contain the same elements in the same ration
law of definite proportions
the ratio of masses of one element that combine with a fixed mass of the other element can be expressed in small whole numbers
law of multiple proportions
contain more than 2 atoms
polyatomic molecules
shows the exact number of atoms of each element in a molecule
molecular formula
shows elemental composition and general arrangements
skeletal formula
whole-number ratio of elements; gives the simplest formula rather than actual formula
empirical formula
substance that consists of just 2 different elements
binary compounds
contain only H and C
hydrocarbons
simplest hydrocarbon
alkanes
compounds without C
inorganic compounds
consists of a combination of two or more ions
polyatomic ions
polyatomic anions that contain one ore more oxygen atoms and once atom of another
oxoanions
produce hydrogen ion an the corresponding oxyanions when dissolved in water
oxoacids
one ionizable hydrogen
monoprotic
more than one ionizable hydrogen
polyprotic
compound that has a specific number of water moles within its solid structure
hydrate
mass in amu of an individual molecule
molecular mass
a list of percent by mass of each element in a compound
percent composition by mass
mass in grams of one mole of a substance
molar mass
atoms will lose, gain, or share electrons in order to achieve a noble gas electron configuration
octet rule
occur between atoms that share electrons
covalent bonds
occur between a metal and a nonmetal and involve ions
ionic bond
bond where electrons are not shared equally
polar
ability of an atom in a compound to draw electrons to itself
electronegativity
a bond between atoms whose electronegativity differ by the range of .5 to 2.0
polar
quantitative measure of the clarity of a bond
dipole moment
comparing calculated dipole moment with measured values gives a quantitive way to describe the nature of a bond
percent ionic character
used to determine the most plausible lewis structure when more than one exist
formal charge
covalent bond in which one of the atoms denotes both electrons
coordinate covalent bond
species that has a lone pair of electrons that can be donated
lewis base
species that can accept a pair of electrons
lewis acid
