Presentation is loading. Please wait.

Presentation is loading. Please wait.

Chem Lewis Structures Exit Quiz next class period Mon 5/8, Tues 5/9

Published byAleesha Strickland Modified over 6 years ago

Similar presentations

Presentation on theme: "Chem Lewis Structures Exit Quiz next class period Mon 5/8, Tues 5/9"— Presentation transcript:

1 Chem Lewis Structures Exit Quiz next class period Mon 5/8, Tues 5/9
Pages 1-4 of SOL Review Packet due next class period.

2 Hybridization Hybridization: combining/mixing of electron orbitals when atoms bond. The hybridization is determined by the # things around the central atom The shape is determined by the lone pairs on the central atom

3 Common Hybridizations
# Sets Orbital Hybridization 2 sp 3 sp2 4 sp3 Note: “sets” refer to bonded atoms as well as lone pairs on the central atom

4 VSEPR Theory Valence Shell Electron Pair Repulsion A=Central Atom
X=Bonded Atoms E=electron pairs (non-bonding) on the central atom

5 These are REFERENCES…not all the possible hybridizations!

6 sp linear Tetra-hedral sp3 sp2 sp3 sp3 bent AX2 AX4 Trigonal planar
AX3E pyramidal sp3 AX2E2 bent

7 sp3 AXE3 linear All diatomic molecules are linear in shape

8 Polarity of Molecules (Compound)
Comparing electronegativity difference between 2 atoms in a bond, for all bonds in the compound If there is an electronegativity difference between bonded atoms, and the molecule is asymmetrical, then the compound is polar

9 Polarity of Molecules If there is an electronegativity difference between bonded atoms, and the molecule is completely symmetrical then the compound is nonpolar

10 Polarity of Molecules If there is no electronegativity difference between bonded atoms, and the molecule is completely symmetrical then the compound is nonpolar

11 linear no polar yes nonpolar yes nonpolar no polar no polar yes nonpolar

12 Intermolecular Forces (sometimes referred to as “Van der Waals forces”)
Attractive forces between molecules are NOT BONDS, which is an attraction between 2 atoms Lots of H2O molecules

13 Types of IMFs: London Dispersion Forces
The weakest intermolecular force Is the main attractive force between nonpolar molecules In general, the larger the molecules, the greater the dispersion forces

14 Types of IMFs Dipole-Dipole Forces Stronger than dispersion forces
The main attractive force between polar molecules

15 Types of IMFs Hydrogen Bonding: is an intermolecular force; it is NOT actually a bond! The strongest intermolecular force Only occur in molecules containing Hydrogen AND one of the following: Nitrogen, Oxygen, or Fluorine (NOF)

16 Practice polar yes Hydrogen bonding London dispersion nonpolar no no
Dipole-dipole polar yes Hydrogen bonding nonpolar no London dispersion

17 32 AX4 nonpolar 8 tetrahedral London dispersion 24 sp3

Download ppt "Chem Lewis Structures Exit Quiz next class period Mon 5/8, Tues 5/9"

Similar presentations

Molecular Shape Sect 9.4. VSEPR Model Valence Shell Electron Pair Repulsion Valence Shell Electron Pair Repulsion Electron pairs will position themselves.

Molecular Shape Sect 9.4. VSEPR Model Valence Shell Electron Pair Repulsion Valence Shell Electron Pair Repulsion Electron pairs will position themselves.
Valence Shell Electron Pair Repulsion Theory

Valence Shell Electron Pair Repulsion Theory
Ch 6.5 Molecular Geometry.

Ch 6.5 Molecular Geometry.
- Lewis structures and bonds - bonding theories

- Lewis structures and bonds - bonding theories
Chapter 16 Notes, part IV Polarity and IMFs. Types of Bonds Up until now, we have assumed that there are two types of bonds: Covalent and Ionic. This.

Chapter 16 Notes, part IV Polarity and IMFs. Types of Bonds Up until now, we have assumed that there are two types of bonds: Covalent and Ionic. This.
IIIIII Molecular Geometry (p. 232 – 236) Ch. 8 – Molecular Structure.

IIIIII Molecular Geometry (p. 232 – 236) Ch. 8 – Molecular Structure.
Polarity of Molecules 11/18/14 Polar Molecules are molecules which have an uneven distribution of charge. One side of the molecule is negative while.

Polarity of Molecules 11/18/14 Polar Molecules are molecules which have an uneven distribution of charge. One side of the molecule is negative while.
Polarity of Bonds & Molecules

Polarity of Bonds & Molecules
Polarity and IMF. Polar Bonds When the atoms in a bond are the same, the electrons are shared equally. This is a nonpolar covalent bond. When two different.

Polarity and IMF. Polar Bonds When the atoms in a bond are the same, the electrons are shared equally. This is a nonpolar covalent bond. When two different.
Molecular Shapes and Polarity 2. Valence Shell Electron Pair Repulsion Theory Also known as VSEPR A theory based on the repulsive forces between valence.

Molecular Shapes and Polarity 2. Valence Shell Electron Pair Repulsion Theory Also known as VSEPR A theory based on the repulsive forces between valence.
Ch-8 review.

Ch-8 review.
Molecular Shape Section 9.4

Molecular Shape Section 9.4
Polarity Chapter 6.1. Review A covalent bond is formed between two non-metals. Electrons are shared. Orbitals are overlapping.

Polarity Chapter 6.1. Review A covalent bond is formed between two non-metals. Electrons are shared. Orbitals are overlapping.
Chemical bonding Bonding Chemical bond – the transfer or sharing of electrons Ionic bond- the transfer of electrons Covalent bonding – the sharing of electrons.

Chemical bonding Bonding Chemical bond – the transfer or sharing of electrons Ionic bond- the transfer of electrons Covalent bonding – the sharing of electrons.
Intermolecular and Intramolecular Forces Review. In the compound PCl 3, how many valence electrons are present? 1.4 2.8 3.24 4.26.

Intermolecular and Intramolecular Forces Review. In the compound PCl 3, how many valence electrons are present?
Bonding Unit Learning Goal #4: Relate the properties of simple compounds to the types of bonding, shape of molecules, and intermolecular forces.

Bonding Unit Learning Goal #4: Relate the properties of simple compounds to the types of bonding, shape of molecules, and intermolecular forces.
Molecular Geometry. 2-D and 3-D Lewis Structures explain the two dimensional structure of molecules In order to model the actual structure of a molecule.

Molecular Geometry. 2-D and 3-D Lewis Structures explain the two dimensional structure of molecules In order to model the actual structure of a molecule.
LEWIS STRUCTURES & MOLCULAR GEOMETRY. TYPES OF COVALENT BONDS SINGLE BONDS LONGEST OF THE 3 TYPES WEAKEST OF THE 3 TYPES CONTAINS ONE PAIR OF ELECTRONS.

LEWIS STRUCTURES & MOLCULAR GEOMETRY. TYPES OF COVALENT BONDS SINGLE BONDS LONGEST OF THE 3 TYPES WEAKEST OF THE 3 TYPES CONTAINS ONE PAIR OF ELECTRONS.
Chemical Bonding Chapter 6. Molecular Geometry VSEPR Valence – Shell, Electron Pair Repulsion Theory.

Chemical Bonding Chapter 6. Molecular Geometry VSEPR Valence – Shell, Electron Pair Repulsion Theory.
Polar Bonds and Molecules Notes. Bond Polarity The bonding pairs of electrons are pulled in a tug-of-war between the nuclei of the atoms sharing the electrons.

Polar Bonds and Molecules Notes. Bond Polarity The bonding pairs of electrons are pulled in a tug-of-war between the nuclei of the atoms sharing the electrons.

Similar presentations

Ads by Google