final Flashcards
electron configuration for ions
- write regular electron configuration
- determine the number of electrons needed to gain or lose to have a stable octet
- write new ion formation
ion formation by transition metals
-transition metals have an outer s2d10 electron congfiguration
-d-block elements lose their s electrons before their d electrons when forming ions
metals that form more than one charge
Cu1+ and Cu2+
Fe2+ and Fe3+
Pb2+ and Pb4+
Sn2+ and Sn4+
ionic bonds
electrostatic forces that hold ions together in ionic compounds
electrostatic forces
attraction between oppositely charged ions
bonds in metals
-valence electrons in metal atoms are a sea of electrons
-mobile
-drifts freely
-bonds consist of attraction between valence electrons and metal ions
-bonds from delocalized electrons
nonpolar covalent bond
the 2 electrons are shared equally between the 2 nuclei
ternary ionic compound bonds
covalent: holds the atoms in the polyatomic ion together
ionic: bonds the metal cation to the negative polyatomic ion
molecule
neutral group of atoms joined by covalent bonds
properties of molecular compounds
-lower melting and boiling points
-soft solids, liquids, and gases at room temp
-do not conduct electricity
VSEPR model
explains molecular shapes for representative elements; negative electron domains repel each other
ABn
A: central atom, bonded to n atoms of B
AB2
linear
AB3
trigonal pyramidal/planar
AB4
tetrahedral
electron domains
electron pairs in a covalent bond
electron geometries
arrangement of electron domains about the central bonding atom of an ABn molecule, includes nonbonding pairs
3 domains
trigonal planar, 120 angle
4 domains
tetrahedral, 109.5 angle
molecular geometry
arrangement of only the atoms in a molecule; nonbonding pairs are not part of the description
what does a molecule’s polarity depend on
shape and nature of bonds
intermolecular forces
forces of attraction between molecules
types of intermolecular forces
dipole-dipole
hydrogen bonds
london dispersion forces
dipole-dipole
delta+ end of a molecule is attracted to delta- end of another molecule
-strongest intermolecular force
-between polar molecules
hydrogen bonds
special type of dipole-dipole
- H-F, H-O, H-N
-large electronegativity
-strong dipole with H delta+
-attracted to unshared electron pairs in other molecules
london dispersion forces
weak intermolecular forces experienced by all atoms and molecules
-electrons constantly in motion
-electron distribution can be uneven
-creates temporary dipoles
alkanes
contains only single bonds (saturated)
alkenes
contains one or more double bonds (unsaturated)
alkynes
contains one or more triple bonds (unsaturated)
stp
standard temperature and pressure
empirical formula
lowest whole number ratio of elements in a compound
acid-base reactions
acid reacts with a base and the two neutralize each other, producing water (sometimes a weak electrolyte)
polyprotic acids
contains more than one ionizable proton and releases them sequentially
hydronium ion
H3O+
oxidation reduction reactions
electrons are transferred from one reactant to another
oxidation
atoms lose electrons
reduction
atoms gain electrons