Chapter 1 Flashcards
Ion purpose:
- Reactivity
- Regulate cellular activity (ex action potential)
EK 3
Alkali Metals: +1
soft
low density
lower melting point
anions, react with nonmetals
can also react with with H and form hydrides (H-)
Highlight reactive–exothermic and explosive in water
ek 7
H:
is used in bonds (intermolecular force)
is important in chemical rxns (acids bases)
ek 7
alkaline earth metals: +2 harder higher melting point higher density less high energy (bc s orbital complete) the heavier the more reactive
ek 7
Group 14
can form 4 covalent bonds with nonmetals
beyond period 2, can also form 2 more bonds in d orbital with LEWIS bases
(so 4:3)
ek 7
Group 15
form 3 covalent bonds
and additionally 2 covalent bonds in d orbital
and 1 more with LEWIS bases
(so 3:3)
or (4:3) because N can form a 4th covalent bond by donating its lone pair of e
ek 7
Group 16 O S can make 2-6 bonds O binds with metals to make metal oxides (alkali earth make peroxides and super oxides) S makes metal sulfides
ek 8
Group 17
highly reactive
radioactively stable
diatomics (like O, N, H)
all can have -1 charge and except F, also +7 (like when paired with very EN atom)
can make more than 1 bond (rare) (F obvs cant)
can combine with H to make hydrogen halides, and are soluble in water and make hydrohalic acids
can combine with metals to make ionic halides
ek 8
Cr and Cu quantum numbers: Instead they borrow one electron from the highest s subshell so they end up with a half-filled s subshell and a half-filled or filled d subshell. This phenomenon is most likely to appear on the MCA’f® with the elements Cr and Cu, which have only one electron in the 4s orbital. The electron configuration of Cr is [Ar] 4s 1 configuration of Cu is [Ar] 4s 1 3cf’0
3d5
Ek 16
Covalent bonds form if their collective energy is less (more stable). Thus, energy is released when bonds are formed. Energy is required/absorbed to break a bond.
EK 23
When electrons are shared equally by two atoms with equivalent electronega-
tivities, it is a nonpolar covalent bond. When the electrons are not shared equally
because of a difference in electronegativity, it is a polar covalent bond. If the dif-
ference in electronegativity is significant, the bond is said to have partial ionic
character.
A bond that has a dipole moment is polar; a bond without a
dipole moment is nonpolar. A molecule with polar bonds may
or may not have a net dipole moment. Since a dipole moment
is a vector, the sum of the dipole moments of the polar bonds
of a molecule can equal zero, leaving the molecule without a
dipole moment, as is the case for symmetrical molecules.
EK 23
transition metals, ions are formed by losing electrons from the subshell with the highest principle quantum number first. Generally this is the s subs hell.
EK 16
Naming Inorganic Compounds
Ionic: cation and anion
- if cation has multiple charges, use roman numerals after name OR ic for more charge and ous for less
- —if cation is made from nonmetal, put -ium at end
- monatomic/simple polyatomic anions end in -ide
- —polyatomic anions with many O’s end in -ite or -ate(more), and if there are four, use hypo at beginning of least and per at beginning of most O molecule
- –and if oxygen anion has H then you say hydrogen first and then name the oxygen part
Molecular Compounds:
- 2 elements (binary): farthest down and left is first element, followed by second
- –second element has -ide at end
- –use number prefix for elements that have multiple atoms
Acids: named for anions
- if anion ends with -ide, then acid starts with “hydro” and ends with “ic”
- with oxyacids, ending “ic” for more o’s and “ous” for less o’s
EK 25
Rate law has rate=k[A][B]
EK 63
Thermodynamics is concerned with and NOT
exothermic and endothermic NOT rate/kinetics
