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AP Chemistry - Chapter 9

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Section 1

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triple covalent bond

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Chemistry Science

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Cards (28)

Section 1

(28 cards)

triple covalent bond

Front

covalent bond where there are only six valence electrons being shared between two atoms

Back

ionic bonding

Front

-a chemical bond (attraction) that is characterized by the transfer of electrons to form ions between metals and non-metals -the amount of energy involved in is calculate using Coulomb's Law

Back

coordinate covalent bond

Front

-where an atom contributes an unshared electron pair (lone pair) to form double or triple bonds to achieve a stable octet around both atoms -sometimes refer to as multiple bond

Back

molar heat formation

Front

the amount of heat involved when 1 mole of compound is formed from its elements

Back

Molar Bond Energy (Enthalpy)

Front

-the energy to required breaking or released from forming one mole of a particular chemical bond -in general, ΔEbond > 0 (endothermic) when breaking a bond ΔEbond <0 (exothermic) when forming a bond

Back

formal charge

Front

-the difference between the number of valence electron of the original atom and the number of valence electron actually assigned to the atom in the Lewis structure -in cases where molecule have more than one possible Lewis structure, the one with the formal charges closest to 0 has the lowest energy --> it is more stable than the other ones

Back

Bond Enthalpiesof Multiple Bonds

Front

in general, bond energy increases with multiple bonds because their length are shorter than single bonds

Back

Lewis Structure

Front

shows electrons of valence electron (s and p orbitals) as dots for all atoms of representative elements (Groups IA to VIIIA). Because it can have max of eight electrons around each atomic symbol, the Lewis Structure cannot be used on transition metals.

Back

determining the Molar Heat of Fomation

Front

ΔH = ∑BE (breaking old bonds) + ∑BE (forming new bonds)

Back

trends in electronegativity

Front

1. electronegativities INCREASE as one move to the right of a period (up to and including halogens) 2. electronegativities DECREASE down the group

Back

Haber-Born Cycle

Front

-a procedure where the energy of every step of the process are accounted for to find the overall energy of the entire process - in the formation of ionic compound, the Haber-Born cycle involves sublimation of metal, ionization of metal into gaseous cation, bond energy of non-metal molecules (if any), electron affinity of non-metal anions, and the lattice energy

Back

resonance

Front

occurs when more than one Lewis structure exists for a molecule

Back

covalent compound

Front

-a compound that consists of only covalent bonds -sometimes refers to as molecular compound

Back

Coulomb's Law

Front

-the energy involved between the charges of two objects as well as the distance between them -lattice energy between ions can be calculated from Coulomb's Law -since energy is released when ionic compounds are formed from ions, lattice energy is exothermic (negative value energy) -similarly, if ionic compounds are dissociated back into ions, the lattice energy will be endothermic (positive value energy) Lattice Energy = -k((Q1Q2)/r) k- electric constant (8.99x10^9 N*m^2/C^2)

Back

model

Front

an attempt to explain how nature works on a small level based in empirical observation in a larger level

Back

odd electron molecules

Front

-when the sum of all valence electrons and any net charges yields an odd number of electrons available -odd electrons molecules do not fit well with the localized electron model because the model deals with pairs of electrons. hence, odd electron molecule are very unstable and very reactive

Back

relative bond polarity

Front

- the difference in electronegativity in a molecule 1. ionic bonds have high bond polarity 2. non-polar covalent bonds have no bond polarity 3. polar covalent bonds have some bond polarity

Back

Covalent bond

Front

an attraction force between two non-metal elements where the sharing of valence electrons is taken place so each atom can achieve the stable duet (for hydrogen) or octet (for other representative elements -ns^2np^6) conditions

Back

Ionic bonds

Front

-a chemical bond (attraction) that is characterized by the transfer of electrons to form ions between metals and non-metals -the resulting attraction between the cation(s) and anion(s) is the ionic bond within an ionic compound

Back

polar covalent bond

Front

a covalent bond where electrons are not evenly distributed, resulting in localized charges at either end

Back

exceptions to the octet rule

Front

1. in the second row, due to the 2s and the 2p orbitals, C, N, O, and F should always follow octet 2. because Be is a metal and B is a metalloid, they are most likely to have fewer than 8 electrons around them - INCOMPLETE OCTET 3. in the 3rd period, heavier atoms towards the right of the Table often satisfy the octet rule. This being said, there are times that they can use the empty 3d orbitals to exceed the 8 electrons limit - EXPANDED OCTET 4. elements in higher row can definitely exceed the octet rule -EXPANDED OCTET

Back

potential energy diagram

Front

Back

Lattice energy

Front

-the energy involved when one mole of an ionic solid is formed from separated gaseous ions -lattice energy is usually exothermic (energy is resealed) M+(g) + X-(g) --> MX(s) Lattice energy < 0

Back

double covalent bond

Front

covalent bond where there are only four valence electrons being shared between two atoms

Back

single covalent bond

Front

covalent bond where there are only two valence electrons being shared between two atoms (also referring as bonding electrons)

Back

Average Molar Bond Energy

Front

the average of an individual molar bond energy from all similar type bonds in a mole of molecule

Back

electronegativity

Front

-first determined by Linus Pauling, it is a measure of the capability of an atom within a molecule to attract shared electrons around itself -the better the atom is able to attract electrins, the higher the electronegativity value -electronegativity of noble gases is 0 as their outer orbitals are filled and do not attract electrons

Back

chemical bond model

Front

chemical bonds are the result when atoms are arranged to achive a lower energy state

Back