Unit 3 Flashcards
hydrogen
H+
lithium
Li+
sodium
Na+
potassium
K+
rubidium
Rb+
cesium
Cs+
beryllium
Be+2
magnesium
Mg+2
calcium
Ca+2
strontium
Sr+2
Barium
Ba+2
aluminum
Al+3
silver
Ag+
nickel
Ni+2
zinc
Zn+2
cadmium
Cd+2
copper (I)
Cu+
copper(II)
Cu+2
iron (II)
Fe+2
iron(III)
Fe+3
tin(II)
Sn+2
tin(IV)
Sn+4
lead(II)
Pb+2
lead(IV)
Pb+4
cobalt(II)
Co+2
cobalt(III)
Co+3
mercury(I)
Hg2 +2
mercury(II)
Hg+2
ammonium
NH4+
suffix change
anions
ide, ite, ate
anions
hydride
H-
fluoride
F-
chloride
Cl-
bromide
Br-
iodide
I-
oxide
O-2
sulfide
S-2
selenide
Se-2
telluride
Te-2
nitride
N-3
phosphide
P-3
nitrate
NO3-
nitrite
NO2-
sulfate
SO4 -2
sulfite
SO3 -2
hydroxide
OH-
acetate
CH3CO2
cyanide
CN-
carbonate
CO3 -2
hypochlorite
CIO-
chlorite
CIO2-
chlorate
CIO3-
perchlorate
CIO4-
chromate
CrO4 -2
dichromate
Cr2O7 -2
permanganate
MnO4 -2
bicarbonate
HCO3-
bisulfate
HSO4-
bisulfite
HSO3-
phosphate
PO4 -3
hydrogen phosphate
HPO4 -2
dihydrogen phosphate
H2PO4-
transfer e-
ionic bonding
metal and nonmetal
ionic bonding
ionic compound
ionic bonding
share e-
covalent bonding
nonmetal and metalloid
covalent bonding
molecular compound
covalent bonding
molecular element (7 diatomic elements)
covalent bonding
size of an atom
atomic radii
we know atoms are what shape
spheres
t or f atoms are all the same size
false
as we move down a group, the atomic radius
increases
as we move across a period from left - right the atomic radius
decreases
why does atomic radius increase as we go down a group
we have a larger number of energy levels and larger atomic radius because of it
why does atomic radii decrease as we move left - right across a period
we have a larger number of protons and electrons
electrons are pulled closer to nucleus
larger attraction
radius smaller
larger attraction
size of monoatomic ions
spheres
what are smaller than their corresponding atoms
cations
what are larger than their corresponding atoms
anions
why are cations smaller than their corresponding atoms
with a smaller number of energy, cation has a smaller radius than its corresponding
extra electrons cause what
some additional repulsions between the electrons
what do electrons do to minimize additional repulsions
expand outward
when electrons expand outward the
radius increases
same number of electrons
isoelectronic series
process of removing an electron from an atom is called
ionization
amount of energy required to remove an electron from an isolated atom in the gas phase
ionization energy
in each period which elements have the largest ionization energy
noble gases
in each period which elements have the smallest ionization energy
alkai metals
in each period which elements have similar ionization energies
transition metals
why do the noble gases have the largest ionization energies in each period
don’t want to lose their NGEC; make removing e- as difficult as possible (large ionization energy)
why do alkai metals have the smallest ionization energies
want to lose electron to get NGEC so make it as easy as possible; making small ionization energy
amount of energy absorbed when an electron is added to an isolated atom in the gas phase
electron affinity
why do the transition metals within a period all have similar ionization energies
lose same e- (same amount of energy, similar ionization energies)
tendency of an atom to attract electrons towards itself when chemically combined with other atoms
electronegativity
atom has a strong desire to attract electrons
large electronegativity
atom has little desire to attract electrons toward itself
small electronegativity
e- are shared equally between the 2 atoms; occurs when 2 atoms involved have the same (or similar) electronegativities
nonpolar covalent bond
small difference in electronegativity
nonpolar covalent bond
electrons are shared but aren’t shared equally
polar covalent bond
occurs when there is a noticeable difference in the electronegativity of the 2 atoms included
polar covalent bond
medium size difference in electronegaitivty
polar covlanet bond
force of attraction between two molecules
intermolecular force
this particular example is an example of a hydrogen bond
intermolecular bond
only occurs when a hydrogen is attracted to either N,O,F
N-H O-H F-H
the smallest electrically neutral collection of ions
formula unit
no difference or very small difference in electronegativities
nonpolar covalent
electrons are shared equally between the two atoms
nonpolar covalent
no charges are present
nonpolar covalent
atoms are connected by covalent bonds
nonpolar covalent
medium size difference in electronegativities
polar covalent
electrons are shared unequally between the two atoms
polar covalent
partial charges are present
polar covalent
atoms are connected by covalent bonds
polar covlanent
large difference in electronegativities
ionic bond
electrons are transferred from one atom to another
ionic
full charges are present
ionic
ions are not connected
ionic bond
