Unit 6 Flashcards
Structural formula
Graphic representations of the relative placement of atoms in a molecule and the bonds between them
Structural formula AKA
Lewis structure
Structural formulas are important to chemists b/c
They can predict behavior by knowing the structural formula of molecules
of electrons in a single bond
2
of electrons in a double bond
4
of electrons in a triple bond
6
Bond dissociation energy
Total energy required to break the bond between 2 covalent bonded atoms
Is breaking a bond exothermic or endothermic?
Endothermic
Forming bonds
Exothermic
Longest to shortest covalent bonds
Single, double, triple
Strongest to weakest bonds
Triple>double>single
Dispersion involves
Temporary dipoles
Dispersion occurs between
Non polar molecules
Dispersion strength of attraction
Low
Dipole-dipole involves
Permanent dipoles
Dipole dipole occurs between
Polar molecules
Dipole dipole strength of attraction
Medium
H bond involves
Permanent dipoles of H, N, O, F
Hydrogen bonding occurs between
Polar molecules
H bond strength of attraction
High
Strength of bonds including ionic
Ionic >hydrogen>dipole dipole>dispersion
Three types of polarities
Ionic, polar covalent, non polar covalent
Determination of bond polarity
The different between the electronegativity of the atoms. If result is between 0.4-1.7, bond is polar covalent
Ionic bonds are always
Polar bonds
Ionic bond electronegativity
Difference greater than 2
Non polar covalent bonds have ____ to ____ electronegativity
Very low to no
All diatomic molecules are
Nonpolar
Diatomic molecules
Br2, I2, N2, Cl2, H2, O2, F2
In nonpolar molecules, the dipoles
Cancel each other
2 molecular shapes that will always produce polar molecules
Bent, trigonal pyramidal
Intermolecular forces
Attractive forces between molecules.
Intermolecular forces are much weaker than
Intramolecular forces
What types of forces/bonds are breaking when water boils?
Intermolecular
What determines whether particles that make up a substance are solids, liquids or gases?
The magnitude (and type) of intermolecular forces.
Weaker than ionic bonds
Covalent
Low meting and boiling points
Covalent
Generally soft and wont shatter
Covalent
Poor conductors of heat and electricity
Covalent
Most are soluble in water
Covalent
Solid, liquid, gas at room temperature
Covalent
Strong bonds
Ionic bond
High melting and boiling points
Ionic bond
Hard and brittle (solid at room temperature)
Ionic bond
Poor conductors in solid state
Ionic bond
Good conductors when molten or dissolved in water
Ionic bond
Soluble in water
Ionic bond
Malleable and ductile
Metallic bonds
Metallic bonds
Solid, high melting points, strong bonds
Isotope
If a compound begins with hydrogen
To name an acid that has no oxygen, the prefix is ___ and the acid name ends in ___
Hyrdo, ic
To name an acid that has oxygen if the compound name ends in -it’s, acid form of the name would end in
Ous
Electrons are ____ in covalent compounds
Shared
The tendency of an atom in a compound to attract electrons
Electronegativity
A kind of bond in which there is unequal sharing of electrons
Polar covalent
Any bond in which there is electron sharing
Covalent bond
The particle formed when 2 or more atoms bond covalently
Molecule
Model that shows how atoms are arranged in a molecule
Structural formula
Model used to determine the molecular shape
VSEPR model
