Go on. Explore!

lvl 0 • 0 xp

lvl 1

Home Market Decks Interests

AP Chemistry Chapter 9 Vocab

memorize.ai (lvl 286)

(0)

27 cards

()

Section 1

Preview this deck

Electronegativity Differences

Front

1 / 27

Chemistry Science

0.0

0 reviews

5			0
4			0
3			0
2			0
1			0

Active users

All-time users

Favorites

Last updated

6 years ago

Date created

Mar 1, 2020

Cards (27)

Section 1

(27 cards)

Electronegativity Differences

Front

Back

Born-Haber Cycle

Front

Relates lattice energies of ionic compounds to ionization energies, electron affinities, and other atomic and molecular properties.

Back

Triple Bond

Front

Two atoms share three pairs of electrons.

Back

Multiple Bonds

Front

Bonds formed when two atoms share two or more pairs of electrons.

Back

Electronegativity

Front

The ability of an atom to attract toward itself the electrons in a chemical bond.

Back

Bond Enthalpy

Front

The enthalpy change required to break a particular bond in one mole of gaseous molecules.

Back

Bond Length

Front

The distance between the nuclei of two covalently bonded atoms in a molecule.

Back

Single Bond

Front

Two atoms are held together by one electron pair.

Back

Lewis Dot Symbol

Front

Consists of the symbol of an element and one dot for each valence electron in an atom of the element.

Back

Double Bond

Front

Two atoms share two pairs of electrons.

Back

Polar Covalent Bond

Front

The electrons spend more time in the vicinity of one atom than the other.

Back

∆H° = ∑BE(reactants) - ∑BE(products) = total energy input - total energy released BE stands for average bond enthalpy ∑ is the summation sign

Front

Equation for Calculating Enthalpy Change of a Reaction from Bond Enthalpies

Back

Formal Charge

Front

The electrical charge difference between the valence electrons in an isolated atom and the number of electrons assigned to that atom in a lewis structure.

Back

Electronegativity Trend

Front

Back

Lewis Structure

Front

A representation of covalent bonding in atoms in which shared electron pairs are shown either as lines or as pairs of dots between two atoms, and lone pairs are shown as pairs of dots on individual atoms.

Back

Resonance Structure

Front

One of two or more lewis structures for a single molecule that cannot be represented accurately by only one lewis structure.

Back

Lone Pairs

Front

Pairs of valence electrons that are not involved in covalent bond formation.

Back

Born-Haber Cycle Example

Front

Back

E α Q_+ x Q_- / r = k x Q_+ x Q_- / r Q are a positive and negative ion k is the proportionality constant r is the distance E is potential energy

Front

Coulomb's Law

Back

Ionic Bond

Front

The electrostatic force that holds ions together in an ionic compound.

Back

https://mgh-images.s3.amazonaws.com/9780072969047/6228-7-38I1.png

Front

Some Bond Enthalpies of Diatomic Molecules and Average Bond Enthalpies for Bonds in Polyatomic Molecules

Back

Resonance

Front

The use of two or more lewis structures to represent a particular molecule.

Back

Covalent Compounds

Front

Compounds that contain only covalent bonds.

Back

Covalent Bond

Front

A bond in which two electrons are shared by two atoms.

Back

Coordinate Covalent Bond

Front

A covalent bond in which one of the atoms donates both electrons.

Back

Octet Rule

Front

An atom other than hydrogen tends to form bonds until it is surrounded by eight valence electrons.

Back

Coulomb's Law

Front

The potential energy (E) between two ions is directly proportional to the product of their changes and inversely proportional to the distance of separation between them.

Back