Unit 3: Chemical Bonding

Question 1

DEF

Answer 1

The mutual electrical attraction between nucei and valence elections of different atoms, occurs when an atom shares, tranfers, or extranges electrons to obtain stability

Question 2

Octet Rule

Answer 2

Fir an atom to become stable it needs to have 8 electrons on its valence shell (outer shell)

Question 3

Ionic Bonding

Answer 3

Electrostatic force of attraction between positive and negative ions

Question 4

Covalent Bonding

Answer 4

The sharing of electron pairs between nonmetal atoms (4 types: polar, nonpolar, coordinate, network)

Question 5

Metallic Bonding

Answer 5

Attraction between metal cations and outer mobile electrons

Question 6

Ion

Answer 6

An atom when it gains or loses electrons

Question 7

Cation

Answer 7

Positively charged ions, lost electrons, become smaller

Question 8

Anion

Answer 8

Negatively charged ions, gained electrons, get bigger

Question 9

Ionic Bonds

Answer 9

One atom gains electrons, one atom loses electrons, a metal and a nonmetal, a metal and a polyatomic ion, there has to be a transfer of electrons, occurs between a metal cation and a nonmetal anion, electronegativity thing

Question 10

Ionic compounds

Answer 10

Compound formed by the electrostatic force of attraction between positive and negative ions

Question 12

Crystal Lattice

Answer 12

3D arrangement of ions

Question 13

Lattice energy

Answer 13

Energy released when one mole of ionic crystalline compound is formed from gaseous ions

Question 14

Properties of Ionic compounds

Answer 14

High melting and boiling points, soluble in water, hard crystalline solids but can fracture, good conductors in liquid or dissolved states, poor conductors in a solid state

Question 15

Covalent bonding

Answer 15

Occurs between nonmetals, they share valnece electrons, most chemical bonds are covalent bonds, 4 types

Question 16

Polar covalent bonds

Answer 16

valence electrons are shared unequally

Question 17

Nonpolar covalent bonds

Answer 17

valence electrons are shared equally

Question 18

Polarity (bond and molecular)

Answer 18

The unequal sharing of electrons, this can happen in individual bonds or an entire molecule

Question 18

Covalent Bonds

Answer 18

A covalent bond forms when the difference between the electronegativities of two atoms is too small for electron transfer to occur to form ions, a molecule is formed from a covalent bond

Question 19

Bond Polarity (Polar)

Answer 19

The electronegativities are slightly unequal causing one atom to attract the electrons more (unequal sharing)

Question 20

Bond Polarity (nonpolar)

Answer 20

The electronegativities are equal and the electrons are shared equally between the atoms

Question 21

Molecular Compound

Answer 21

Neutral compound consisting of nonmetals covalently bonded (ex. CO2, HCI)

Question 22

Molecule

Answer 22

Smallest representative unit of a molecular compound; can exist independently (ex. O2, Cl2, H2)

Question 23

Diatomic Molecules

Answer 23

Molecules consisting of two atoms of the same element covalently bonded, “HOFBrINCl”

Question 24

Bond Length

Answer 24

Adverage distance between nucelei of two bonded nonmetal atoms (sum of atomic radii)

Question 25

Coordinate Covalent Bond

Answer 25

Results when both electrons shared in the covalent bond come from one of the atoms

Question 25

Bond Angle

Answer 25

Angle between two bonds in a molecule

Question 26

Bond Energy

Answer 26

The energy needed to break a bond and form a new bond

Question 27

Single Bond

Answer 27

Weakest bond, longest bond, least amount of energy

Question 28

Double Bond

Answer 28

In between a single and triple bond on everything

Question 29

Triple Bond

Answer 29

Strongest bond, shortest bond, most amount of energy

Question 30

Coordinate covalent bond (polyatomic ion)

Answer 30

Covalently bonded atoms with an overall charge, since they have an overall charge, they can form ionic bonds with other ions, ex. hydroxide ion, carbonate ion

Question 31

Network Covalent bond

Answer 31

3D network of covalently bonded atoms that extend in all directions to make large crystalline structures, ex. graphite, diamond

Question 32

Network solids properties

Answer 32

Strong bonds (very high melting/boiling points, solid at room temperature), insoluble in water, nonconductor

Question 33

Molecule properties

Answer 33

Gases or dull brittle solids, poor conductors of heat and electricity(because electrons are stuck in the bonds and cannot move), low melting/boiling points (weak bonds and easy to break requiring little energy), solubility depends on “like dissolves like” (polar substances will dissolve other polar substances, nonpolar substances will dissolve in other nonpolar substances)

Question 34

VSEPR Theory

Answer 34

Valence shell electron pair repulsion, electron pairs spread as afar apart as possible to minimize repulsive forces