Chapter 6-Bonding Flashcards by Sarah Porter

All things in nature favor arrangements that _________ potential energy

Minimize

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Chemical bond

Mutual attraction between the nuclei and the valence electrons of different atoms that binds the atoms together

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Molecules have ______ potential energy than individual atoms

Lower

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Covalent bonding

The two atoms in a covalent bond share valence electrons

Typically seen when nonmetal atoms bond to other nonmetal atoms

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Ionic bonding

One atom gains electrons and the other atom loses electrons, forming ions which attract each other
Electrons are not shared
Typically seen when metal atoms bond to nonmetal atoms

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A covalent compound is a

Molecular compound

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Covalent compounds can be

Solid liquid or gas
Low melting points
Do not conduct electricity

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Nonpolar covalent bonding

Electrons are shared equally

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Polar covalent bonding

Electrons are not shared equally

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In a purely ionic bond

Electrons are not shared at all

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100% ionic character means

Completely ionic

Electrons are not shared at all

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0% ionic character means

Completely covalent

Electrons are shared completely equally

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If two atoms in a covalent bond have equal electronegativities, then

They would share electrons equally, forming a Nonpolar bond

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If two atoms in a covalent bond have different electronegativities, then

They will share electrons unequally, forming a polar bond

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When electrons are shared unequally,

It creates a partial charge around the atoms in the bond

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Atoms with higher electronegativities will attract electrons more strongly and therefore

Take on a partially negative charge

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Atoms with lower electronegativities will attract electrons less strongly and therefore

Take on a partially positive charge

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Nonpolar covalent compound

Molecules that are jot attracted to a charge

Contains only Nonpolar bonds or contains polar bonds that cancel each other out

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Polar covalent compounds

Are attracted to a charge

Contains polar bonds that do not cancel each other out

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Ionic bonding

Chemical bonding that results from the electrical attraction between cations and anions

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Covalent bonding

Sharing of the electron pairs between two atoms

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Molecule

A neutral group of atoms that are held together by covalent bonds

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Ionic compounds typically form

Crystalline solids

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Ionic compounds are

Solid at room temperature
Have high melting points
Most are crystalline solids

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Electrolytes

The solutions of ionic compounds that will conduct electricity

Dissociation

When an ionic compound dissolves in water, breaking apart into its constituent ions

Ionic bonds/compounds physical properties

Dissociates into ions when dissolved in water Solution can conduct a current Ionic compounds are electrolytes

Covalent bonds/compounds physical properties

Does not dissociate when dissolved in water Solution cannot conduct a current Covalent compounds are nonelectrolytes

A single covalent bond consists of _______ pair of shared valence electrons (two electrons total)

One

A double bond consists of ___ pairs of shared electrons (four total)

Two

A triple bond consists of ____ pairs of shared electrons (six total)

Three

Bond strength | _______bonds>_______bonds>_______bonds

Triple,double,single

Bond energy | _______bonds>_______bonds>_______bonds

Triple,double,single

Bond length | _______bonds>_______bonds>_______bonds

Single,double,triple

Bond______ and bond_______ are directly proportional

Bond Strength and bond energy

Bond strength and bond energy are inversely proportional to bond_______

Length

Lewis structures are diagrams that show the shared and unshared ____________ in a ________

Valence electrons | Molecule

Shared electrons are typically called

Bonded pairs

Unshared electrons are typically called

Lone pairs

Honc 1234 rule

Hydrogen and the Halogens can form 1 covalent bond Oxygen can form 2 covalent bonds Nitrogen can form 3 covalent bonds Carbon can form 4 covalent bonds

Poly atomic ion

A group of covalently bonded atoms with a charge on the group of atoms as a whole

Most polyatomic ions are negatively charged and will form ionic bonds with

Metal cations

Isomers

Same chemical formula | Different structural formulas

VSEPR stands for

Valence She'll Electron Pair Repulsion

The pairs of valence electrons in a molecule __________ each other

Repel

The paired valence electrons orient themselves as far apart from each other as possible. It is this repulsive force that determines

The shape of the molecule

Electron domain

The space occupied by valence electrons in a molecule, either a bonded pair or a lone pair - affects overall shape of the molecule

Bonded pairs are always

Equidistant

Double and triple bonds count as

One electron domain

A single atom is described as a

Point

Hybrid orbitals

A blend of two or more orbitals on the same atom

Alloys

Mixture of metals Steel Bronze Brass

Bond energy

The amount of energy needed to break a chemical bond OR the amount of energy stored in a chemical bond

INTERmolecular forces

Forces between molecules

INTRAmolecular forces

Forces within a molecule

Intermolecular forces are ___________ than intramolecular forces

Weaker

Hydrogen bonding

Occurs between polar molecules | Strongest of intermolecular forces

When a hydrogen atom is bonded to a highly electronegative atom the hydrogen atom

Takes on a partial positive charge, which means it will be attracted to partially negative atoms of other molecules

An example of a network covalent bond is

A diamond

Metallic bonds are also known as

"Sea of electrons"

``` Linear (3 atoms) # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom: 2 # of bonded pairs around central atom: 2 # of lone pairs around central atom: 0 Bond angle(s): 180 Central atom hybridization: sp ```

``` Trigonal planar # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom: 3 # of bonded pairs around central atom: 3 # of lone pairs around central atom: 0 Bond angle(s): 120 Central atom hybridization: sp2 ```

``` Tetrahedral # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom: 4 # of bonded pairs around central atom: 4 # of lone pairs around central atom: 0 Bond angle(s): 109.5 Central atom hybridization: sp3 ```

``` Trigonal pyramidal # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom: 4 # of bonded pairs around central atom: 3 # of lone pairs around central atom: 1 Bond angle(s): ~107 Central atom hybridization: sp3 ```

``` Bent # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom:4 # of bonded pairs around central atom:2 # of lone pairs around central atom:2 Bond angle(s):~105 Central atom hybridization:sp3 ```

``` Linear (2 atoms) # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom:4 # of bonded pairs around central atom:1 # of lone pairs around central atom:3 Bond angle(s):180 Central atom hybridization:sp3 ```

``` Trigonal bipyramidal # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom:5 # of bonded pairs around central atom:5 # of lone pairs around central atom:0 Bond angle(s):180,120,90 Central atom hybridization:sp3d ```

``` Octahedral # of electron domains around central atom: # of bonded pairs around central atom: # of lone pairs around central atom: Bond angle(s): Central atom hybridization: ```

``` # of electron domains around central atom:6 # of bonded pairs around central atom:6 # of lone pairs around central atom:0 Bond angle(s):180,90 Central atom hybridization:sp3d2 ```

A condition that occurs when more than one valid lewis structure can be written for a molecule is called

Resonance

A double covalent bond involves

Sharing of four electrons

A molecule that has three bonded atoms and one lone pair around the central atom is

Trigonal pyramidal