Chem Bond, Lewis, Naming Flashcards
What is the process of ionic bonding?
Valence electrons are transferred between a metal and a non-metal to achieve the octet
What is a polyatomic ion?
A molecular compound that has an excess or deficit of electrons and thus has a charge.
Why do bonds bond together (other than octet, think charges)
They must combine with oppositely charged ions to achieve a neutral charge.
What is covalent bonding?
Electrons are shared between atoms because the electronegativity difference is not strong enough to completely pull valence electrons away.
What is indicated by arrows in polar covalent bonds?
The direction of electron pulling, pointing to the more electronegative atom.
Fill in the blank: The electronegativity difference for ionic bonding is greater than _______.
1.7
What must bonds do to ensure atoms achieve stability?
Give each atom 8 electrons.
Fill in the blank: The electronegativity difference for POLAR covalent bonding is between _______.
0.5 to 1.69
Fill in the blank: The electronegativity difference for NON-polar (or just covalent) bonding is below _______.
0.5
difference in electron sharing between ionic, polar covalent, and non-polar covalent bonds
i: electrons are transferred, pc: partially shared/unequal, n-pc: shared equally
define single, double, and triple bond
single bond: results from covalent bond sharing ONE pair of electrons (H and H)
double bond: sharing TWO pairs (C and O)
triple bond: sharing THREE pairs (N and N)
define bonding pair and lone pair
bonding: a pair pf electrons that is shared between 2 atoms
lone: a pair of electrons that is NOT shared
Where do H and F go in a Lewis structure
ALWAYS at the end
which goes in the center? most electropositive or most electronegative?
most electropositive
What makes a lewis structure bent?
if there’s a lone pair on the CENTRAL atom, doesn’t matter the #, it will make the structure bend (repulsion)
what is the math letters and meaning for doing Lewis structures
V = valence
T = total
S = shared bonds
NB = non-bonding pair
explain the written math steps for Lewis structure (NF3)
ex. NF3
1. (V) det total valence electrons in all atoms at start [N: 1(5) / F: 3(7)] = 26
- (T) det total # of electrons needed to reach octet
[N: 1(8) / F: 3(8)] = 32 - (S) T-V= Answer /2
[32 - 26 = 6 / 2 = 3 bonding pairs] - (NB) V-S= Answer / 2
[26 - 6 = 20 / 2 = 10 lone pairs]
Which 2 elements have a special octet total # and what is the number?
S = 12, P = 10
Between 2 compounds, how do you know which one has a greater intermolecular force?
- identify what intermolecular force each uses, may be able to determine from that
- both LDF? check molecular weight. The larger one is your answer.
- for dipole-dipole, its the one with the higher EN difference
What are the types of intermolecular forces? (4)
ion-dipole, dipole-dipole, hydrogen bond, London dispersion force or Van der Waals forces
What is a hydrogen bond? example?
A dipole bond between H and O, F, or N. It is the strongest type of intermolecular bond. H2O, HF, strong because high electronegativity difference
types of intramolecular bonds
ionic , polar covalent, or covalent!
Describe London Dispersion Forces?
Weak forces present in non-polar molecules that strengthen as the size of the molecule increases, and disperse very quickly. Its basically imbalance in the electron cloud and all bonds do this atleast slightly.
Fill in the blank: Solubility follows the principle of _______.
Like Dissolves Like.
