Basic Concepts of chemical bonding Flashcards
Order of bond from strongest to weakest
Triple bond < double bond < single bond
Delta H is negative when?
When new bonds are formed
What are the most electronegativity elements?
N,O,Cl,F (F is the most electronegative)
What law is used to determine the amount of lattice energy?
Coulomb’s law: kq1q2/d
How do you determine which lewis structure is most important ?
- The one where the formal charge of the atom is closest to zero
- The lewis structure where the negative charges are on the most eletronegavity atoms
Dimization
When two unstable atoms combine with each other to become stable
Metals have low ______?
Ionization energy
Chemical bonding
The force of attraction between opposite electrical charges and the repulsion between like charges
Delta H is positive when?
Bonds are being broken apart
Nonmetals have high _____?
electron affinity
Lattice Energy increases when what happens?
When the charges on the ions increase and the radi size decreases
Order of bonds from longest to shortest
Single bond < double bond < triple bond
Covalent bonds
The sharing of electrons between two nonmetals
Polar covalent Bonding
Where its neither ionic or covalent
Bond order
Number from 1,2,3 ( Based on typr of bond if single bond bond order is 1 )
Ionic Bonds
The electrostatic forces that exist between oppositely charged particles when one or more valence electrons is transfered (Transfer of electrons between metal & nonmetals)
Octect Rule
Atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons
Lattice Energy
Is the energy required to completely separate one mole of a solid ionic compound into its gaseous ions
Hypervalent
Molecules & ions with more than an octect of electrons around the central atom
How do you determine the formal charge?
Valence # - (# of bond + lone electrons)
Bond enthaply
Is the enthaply change for breaking a particular bond in one mole of gaseous substances
