Topic 2- Lecture 7 Flashcards
Created when a metallic cation forms an electrostatic bond with a nonmetal anion
Ionic compound
These elements lose electrons from their highest s sub level first
D block cations
Metals have a ___________ charge
Positive
Bond that transfers electrons
Ionic
Ionic bonds form…
Positive and negative ions
Metals in an ionic bond form…
Cations
Positive
Lose electrons
Nonmetals in an ionic bond form…
Anions
Negative
Gain electrons
Cations and anions form electrostatic bonds based on…
Opposite charges
Ionic bonds are very strong and take a lot of _________ to break apart
Energy
Bond energy
Input of energy into an ionic bond
Endothermic
Larger ions form…
Weaker bonds
Lower electronegativity =
Closer to each other
More covalent
- strong force of attraction
- high melting point
- very hard
- low volatility (don’t evaporate well)
Ionic solids
Cleave along planes and line up in repetitive pattern to minimize repulsive forces
Don’t bend or stretch
Soluble in polar solvents
Properties of ionic solids
One atom shares one or more pairs of electrons with another atom so they both acquire full octets
Covalent bonds
Bond that occurs between two Nonmetals
Covalent
Electronegativity difference= 0-.5
Balance of shared electrons
Nonpolar covalent bond
Electronegativity difference = .5-1.9
Imbalance of shared electrons
Polar covalent bond
Electronegativity difference =1.9-3.5
Ionic bond
- find total amount of valence electrons
- central atom is least electronegative
- assign single bonds to terminal atoms
- fill in octets of terminal atoms
- extra electrons go on central atom
- use multiple bonds to fill central atom if needed
Lewis structure
Two or more Nonmetals bonded together to form a compound
Bonds are nonpolar/polar covalent
Molecule
Combination of Nonmetals or metals and Nonmetals bonded together
Polyatomic ions
More covalent= __________ electronegativity
Closer in
More ionic= ___________ in electronegativity
Farther apart
Greater electronegativity= more…
Polar
Elements tend to gain, lose, or share electrons to acquire a full shell
The octet rule
