Unit 4 #1 Flashcards
ionic bonds
giving and losing, positive or negative ions, (ex: sodium chloride, sodium becomes positive, chlorine becomes negative)
IMPORTANT THINGY!
atoms want to be a lower energy state (sometimes when two atoms come together, it is because when they are seperated, they are at a higher energy state than together)
covalent bond
(ex: 2 hydrogen atoms comes together and share electrons and become H2), SHARING ELECTRONS
bond energy
the energy required to break a bond
colulmobus law
used to calculate the bond energy
electronegativity
the ability of an atom in a molecule to attract shared electrons to itself
the electron negativey in a periodic table
increaes as you go RIGHT and UP
if the electronegativity is big….
it is ionic
if the electronegantivity is small/ zero
covalent
if the electrogneativity is intermediate
it is a polar covalent
dipolar
molecule that has a center of positive and center of negative charge
the size of atoms periodic table
- down: size increaes
- side to side: depends on atomic number and what group you are in
- AS ATOMIC NUMBER INCREASES, SIZE DECREASES
localized electron bonding model (LE model)
a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bond atoms (electrons in bonding pairs and lone pairs)
electrons in bonding pairs
shared between atoms
lone pairs
not shared
the goal of LE model
to describe the structure of valence electrons
“ane”
all single bonds
“ene”
contains one double bond
“yne”
contains one triple bond
formula charges
number of valence electrons in element minus number of valence electrons assigned to the atom in the molecule (cannot double count covalent bonds)
IMPORTANT THINGY #2
atoms in molecules try to achieve a formula charge as close to 0 as possible, any negative charge should go to the more electrognetaive element
polarity
it increases as the difference in elecronegativity increases
two nonmetals
form covalent bonds
a nonmetal and a representative-groiup metal group
binary ionic compound
cation
lost
anion
gain
