Exam 4 Flashcards
Alkali Metals
- Group 1A
- Increase in reactivity as you move down group
Alkaline Earth Metals
- Group 2A
- Increase in reactivity as you move down group
Halogens
- Group 7A
- Reactivity decreases down group
Noble Gases
- Group 8A
- Very low reactivity
3 Most Abundant Elements in Earth’s Crust
Al, O and Si
Lipitor
Lowers cholesterol by inhibiting HMG-CoA reductase
Building Blocks of Living Organisms
C, O and N
Effective Nuclear Charge
Increases across a period
-Valence electrons attracted by nucleus are also repelled by core electrons
Atomic Radii
-Increase down a group
-Decreases across a period
Cations are smaller
Anions are bigger
Isoelectronic Ions
Atoms of different elements with the same number of electrons
Ionization Energy
Minimum energy required to remove an electron from ground state
- Increases across a period
- Decreases down a group
Exceptions to the Octet Rule
- Always true for C, O and F
- Atoms 3rd period and below have more than 8
- Some atoms, usually 3A, have fewer than 8
Atoms surrounded by an odd number of electrons
Free radical
A dominant resonance structure is one that
- Maximizes number of electrons with formal charge of 0
- Has a negative charge residing on the more electronegative atom
Electronegativity
Increases across a period
Decreases down group
2 bonds, 0 lone pairs
Linear
180
3 bonds, 0 lone pairs
Triangular planar
120
2 bonds, 1 lone pair
Bent
Less than 120
4 bonds, 0 lone pairs
Tetrahedral
109.5
3 bonds, 1 lone pair
Triangular pyramidal
107.5
2 bonds, 2 lone pairs
Bent
104.5
5 bonds, 0 lone pairs
Triangular bypyramidal
90 and 120`
4 bonds, 1 lone pair
Seesaw
3 bonds, 2 lone pairs
T shape
2 bonds, 3 lone pairs
Linear
6 bonds, 0 lone pairs
Octahedral
90
5 bonds, 1 lone pair
Square pyramid
4 bonds, 2 lone pairs
Square planar
Hybridization:2
sp
linear
Hybridization: 3
sp2
triangular planar
Hybridization: 4
sp3
tetrahedral
Hybridization: 5
sp3d
triangular bipyramidal
Hybridization: 6
sp3d2
octahedral
Sigma bond
Head to head overlap
Pi bond
Side by side overlap
Single Bonds
Always sigma bonds
Multiple bonds
One bond is sigma and the rest are pi
Nonpolar Molecules
- Has one of the 5 basic geometries
- Terminal atoms are distributed symmetrically
Polar Molecules
If dipoles do not cancel out
Molecules with only 1 polar bond
