clicker #1 how many unpaired electrons and valence electrons does se have? a) 0; 14 b) 2; 6 c) 2; 14...
DESCRIPTION
Atomic Trends Atomic Radius: size of the orbital H F Fr decreasing increasing More protons = more attraction and smaller radius Orbitals are getting bigger and further from nucleusTRANSCRIPT
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?