Chapter 5 Flashcards
general terms
compound
a substance that is made up of 2 or more different elements combined together chemically. eg- NaCl
molecule
a group of atoms joined together. the smallest particle of an element or compound that can exist independently. eg- Cl2
octet rule exceptions
- transition metals
- hydrogen, lithium, beryllium tend to achieve 2 electrons in their outer shell rather than 8.
ion
a charged atom or group of atoms
ionic bond
force of attraction between oppositely charged ions in a compound. always formed between the complete transfer of electrons from one atom to another.
charges of ionic compounds
g1- 1+
g2- 2+
g3- 3+
g4- 4+ or 4-
g5- 3-
g6- 2-
g7- 1-
g8- no ion
7 diatomic molecules
hydrogen, nitrogen, fluoride, oxygen, iodine, chloride, bromine
H2, N2, F2, O2, I2, Cl2, Br2
transition metals
element that forms at least one ion with a partially filled sublevel. properties:
-have variable valency
-widely used as compounds
-usually coloured compounds
exceptions to transition metals
Sc3+, Zn2+ because they do not have a partially filled d sub-level
what forms a single bond
when one pair of electrons is being shared between 2 atoms
what forms a double bond
when two pairs of electrons are shared between 2 atoms
what forms a triple bond
when three pairs of electrons are shared between 2 atoms
what shape are all double and triple bonds
linear in shape and single
what are the bond energies for single, double, and triple bonds like
single- weakest
double- stronger than single
triple- strongest
~ this is due to sigma bonds being stronger than pi bonds
sigma bond
formed by the head on overlap of 2 orbitals
pi bond
formed by the sideways overlap of p orbitals
how many sigma and pi bonds in each of the 3 bonds
single bond- one sigma bond
double bond- one sigma bond and one pi bond
triple bond- one sigma bond and 2 pi bonds
properties of ionic bonds
-contains a network of ions in the crystal
-usually hand and brittle
-high melting and boiling points
-usually solid at room temp
-conduct electricity when in molten state or when dissolved in water
properties of covalent bonds
-contain individual molecules
-usually soft
-low melting and boiling points
-usually liquids, gasses or soft solids at room temp
-do not conduct electricity
electronegativity
the relative attraction that an atom in a molecule has for a shared pair of electrons in a covalent bond
uses of electronegativity
- predict polarity of covalent bonds
- predict which compounds are ionic and which are covalent
polar covalent bond
a bond in which there is an unequal sharing of the pair(s) of electrons. this causes one side to be slightly positive and the other slightly negative.
non-polar covalent bond
a bond in which there is an equal sharing of electrons
electronegativity difference greater than 1.7 means
ionic bonding