Chp 1: Electron/Molecular Geometry and Polarity

These flashcards cover key concepts related to molecular geometry, electron groups, and polarity, as discussed in the organic chemistry lecture.

The geometry for two electron groups is __.

linear.

The bond angle for a linear geometry is __ degrees.

180.

Carbon dioxide is an example of a __ molecular geometry.

linear.

When three electron groups are all bonding groups, the molecular geometry is __.

trigonal planar.

The bond angle in a trigonal planar geometry is __ degrees.

120.

If there are three electron groups with two bonding groups and one lone pair, the molecular geometry is __.

bent.

For four electron groups where all are bonding, the geometry is __.

tetrahedral.

The bond angle in a tetrahedral geometry is approximately __ degrees.

109.5.

When a molecule has lone pairs, it will distort the bond angle, causing it to be __ than expected.

less.

In organic chemistry, we mainly consider central atoms with __ electron groups.

two, three, or four.

The term used to describe the geometry that considers only the electron groups is __ geometry.

electron.

Molecular geometry specifically considers and of groups.

bonding groups; lone pairs.

If a geometry is trigonal planar and one group is a lone pair, it's called __ molecular geometry.

bent.

The presence of a lone pair results in more electron density, which __ bond angles.

decreases.

London dispersion forces are exhibited predominantly by __ compounds.

nonpolar.

The strongest type of intermolecular force is __ bonding.

hydrogen.

A molecule is __ if it has a central atom with a lone pair.

polar.

All hydrocarbons are generally considered to be __.

nonpolar.

The interactions between polar molecules are called __ forces.

dipole-dipole.

Hydrogen bonds must involve __ atoms (H, N, or O).

hydrogen.

The __ of the carbon dioxide molecule is symmetrical, leading to nonpolar character.

geometry.

For a molecule to be polar, it must have at least one __ bond.

polar.

A __ bond occurs between hydrogen and highly electronegative atoms like O or N.

hydrogen.

When a molecule has an uneven electron cloud due to its shape, it's considered __.

polar.

All compounds exhibit at least some form of __ forces.

intermolecular.

The type of electron cloud distribution affects the __ of the compound.

boiling point.

If a compound has hydrogen bonding, it will generally have a __ boiling point.

higher.

moments that are equal in all directions will result in a nonpolar molecule.

Dipole.

The ability for hydrogen bonding leads to __ in water's properties.

unique characteristics.

The geometry is __, not flat, in compounds with four electron groups.

tetrahedral.

For molecular geometry, a central atom surrounded by four identical atoms will be __ if there are no lone pairs.

nonpolar.

The most significant factor for boiling point among nonpolar substances is __.

atomic size.

A molecule can exhibit __ forces only if it is nonpolar.

London dispersion.

Carbon bonded to four hydrogens (like in methane) is an example of __ bonding.

nonpolar.

The interactions in a liquid sample are due to __ forces.

intermolecular.

The larger the atomic size, the stronger the __ forces will be for nonpolar molecules.

dispersion.

The molecular geometry of a carbon bonded to three identical electronegative atoms and one hydrogen will be __.

polar.

The __ principle explains how molecules orient to minimize repulsion between electron groups.

VSEPR.