Organic Chemistry Chp 1: 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.