clicker #1 how many unpaired electrons and valence electrons does se have? a) 0; 14 b) 2; 6 c) 2; 14...

Clicker #1How many unpaired electrons and valence electrons does Se have?

A) 0; 14B) 2; 6 C) 2; 14 D) 0; 6E) 2; 4

Atomic Trends Atomic Radius: size of the orbital

H F

Fr

decreasing

increasing

Atomic Trends Atomic Radius: size of the orbital

H F

Fr

decreasing

increasingMore protons = more attraction and smaller radius

Orbitals are getting bigger and further from nucleus

Clicker #2Which of the following elements has the largest atomic radius?

A) CaB) AlC) ND) SrE) F

Atomic Trends Ionization Energy

H F

Fr

increasing

decreasing

Atomic Trends Ionization Energy

H F

Fr

increasing

decreasingElectron is at its lowest energy state when closest to the nucleustakes more energy to take an electron away when closer to the nucleus

Clicker #3Which of the following elements has the largest ionization energy?

A) PB) AlC) ClD) BaE) K

Isoelectronic Series Same number of electrons

Example:Which is larger Na+ or Ne?

Isoelectronic Series Same number of electrons

Example:Which is larger Na+ or Ne?

Same number of electrons but Na+ has 11 protons and Ne has 10 protons.

ExampleWhich is larger Cl- or Ar?

Which has a higher ionization energy Cl- or Ar?

ExampleWhich is larger Cl- or Ar?

Which has a higher ionization energy Cl- or Ar?

BONDING “Forces”

What is meant by a “chemical bond”? Why do atoms bond to form

molecules? How do atoms bond to form

molecules?

BONDING Two Types of Bonding

Intramolecular (within a molecule) Intermolecular (between molecules)

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Ionic Compounds Between a metal and a nonmetal

Example: NaClNa: [Ne]3s1

Cl: [Ne]3s23p5

Ionic Compounds Between a metal and a nonmetal

Example: NaClNa: [Ne]3s1 Na+: [Ne]Cl: [Ne]3s23p5 Cl-: [Ne]

3s23p6

Mg -> Mg+ -> Mg2+

Ionization energies of atoms are highly endothermic

HOWEVER… Takes more energy to remove 2nd

electron Once you get Mg2+ (noble gas

configuration) gives off energyOVERALL = EXOTHERMIC PROCESS

Bonding in H2

Is this ionic?

Bonding in H2

Covalent Bonding Sharing electrons Hydrogens share the electrons and

have noble gas configuration

Why isn’t He diatomic?

Bonding in H2

Covalent Bonding Sharing electrons Hydrogens share the electrons and

have noble gas configuration

Why isn’t He diatomic? Already has a noble gas configuration

Therefore… Covalent bonding has same idea as

ionic bonding…

But

Neither atom is “strong” enough to remove electron from the other atom

What about CO?