Chemical Bonding
What is a bond?
2 types of bonds:
electronegativity- when an element gains/gives an electron to be like noble gases
measure the strength of a bond by destroying the bond; the more energy it takes to destroy it, the stronger the bond
bond energy- the amount of energy it takes to break a bond
ionic compound- a positive metal and a negative nonmetal
higher electronegativity equals more negative number
Dipole moment- the magnitudes of separated charges times the distance between the charges
any diatomic molecule that has a polar bond has a dipole moment
H C
2.1 2.5 =0.4
------------->
H P
2.1 2.2 = 0.1
------------->
draw an arrow from positive to negative
magnitude- difference between the number (ex. 0.4 and 0.1)
polar- different charge
polar covalent- share electron but not equally
Properties of ionic compounds:
8 electrons in a Valence shell except for Hydrogen and Helium (they have 2)
Valence- SPDF
Molecular Structure- the three dimensional arrangement of the atoms in the molecule
VSEPR- Valence Shell Electron Pair Repulsion
electrons repel each other because of negative charge
- a force that holds groups of two or more atoms together and makes them functional as a unit
2 types of bonds:
- Covalent bond- shares electrons equally; stronger bond
- Ionic bond- the positive and negative attraction between atoms
electronegativity- when an element gains/gives an electron to be like noble gases
measure the strength of a bond by destroying the bond; the more energy it takes to destroy it, the stronger the bond
bond energy- the amount of energy it takes to break a bond
ionic compound- a positive metal and a negative nonmetal
higher electronegativity equals more negative number
Dipole moment- the magnitudes of separated charges times the distance between the charges
any diatomic molecule that has a polar bond has a dipole moment
H C
2.1 2.5 =0.4
------------->
H P
2.1 2.2 = 0.1
------------->
draw an arrow from positive to negative
magnitude- difference between the number (ex. 0.4 and 0.1)
polar- different charge
polar covalent- share electron but not equally
Properties of ionic compounds:
- they form small crystals
- crystal lattice- the arrangement of ions in an ionic crystal
8 electrons in a Valence shell except for Hydrogen and Helium (they have 2)
Valence- SPDF
Molecular Structure- the three dimensional arrangement of the atoms in the molecule
VSEPR- Valence Shell Electron Pair Repulsion
electrons repel each other because of negative charge
Electron Pair arrangement
1. Linear 2. Trigonal Planer 3. Tetrahedral 4. Tetrahedral 5. Tetrahedral |
Molecular Structure
1. Linear 2. Trigonal Planer 3. Tetrahedral 4. Trigonal Pyramid 5. Bent |
Angle Degree
1. 180 2. 120 3. 109.5 4. 109.5 5. 109.5 |
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