Hesi - Chemical Reactions, Bonds & Interactions

Front 1

Five types of Chemical Reactions?

Back 1

Synthesis, Decomposition, Combustion, Single Replacement & Double Replacement.

Front 2

Chemical Reaction: Synthesis?

Back 2

Two element combine to form a product.

Ex: 2K + 2Cl = 2KCL (Potassium + Chloride = Potassium Chloride)

Front 3

Chemical Reaction: Decomposition?

Back 3

The opposite of Synthesis; breaking a compound into its component parts.

Ex: NaCl --> Na + Cl (when placed in an aqueous solution, table salt decomposes into an ionic solution of Na (cation) and Cl (anion).

Front 4

Chemical Reaction: Combustion?

Back 4

Self-sustaining, exothermic chemical reaction usually initiated by heat acting on oxygen and a fuel compound.

Ex: Ethane: 2C2H6 + 7O2 -> 4CO2 + 6H20 or Ethane + oxygen = CO2 & H20

Front 5

Chemical Reaction: Single Replacement?

Back 5

(Bad date) Involve ionic compounds; a more active metal reacting with an ionic compound containing a less active metal to produce a new compound (whether the reaction takes place is based on the reactivity of the involved metals).
Ex: copper wire & AgNO3 (copper & silver swap places)

Cu (s) + 2AgNO3 (aq) -> Cu(NO3)2 (aq) + 2Ag (s)

Front 6

Chemical Reaction: Double Replacement?

Back 6

(Swingers) Involves two ionic compounds; The + ion from one combines with the - ion from the other = two new ionic compounds that have switched partners.

Ex: AgNO3 + KCl -> AgCl + KNO3

Front 7

Ionic Bonding?

Back 7

Electrostatic attraction between two oppositely charged ions (cation + anion).

Generally formed between a metal and a nonmetal.

Ex: salt Na+ + Cl- = NaCl

Front 8

Covalent Bonding?

Back 8

Formed when two atoms share electrons, generally in pairs, one from each atom.

Strongest of all chemical bonds, generally formed between two nonmetals.

Single CB: One pair; Double CB: Two pairs; Triple: Three pairs

Front 9

Nonpolar Covalent Bond?

Back 9

CB where the electrons in the bond are shared equally.

Front 10

Polar Covalent Bond?

Back 10

The shared electron density of the bond is concentrated around one atom more than the other. Polarity is based on the difference in electronegativity values for the elements involved in the bond. The greater the difference, the more polar the bond will be (one side of the molecule will have a charge distinctly more + and the other side will be more - in charge).

Front 11

Intermolecular Forces?

Back 11

Not bonding interactions; weaker forces of attraction between whole molecules.

Includes: Hydrogen bonds; Dipole-Dipole Interactions & Dispersion Forces.

Front 12

Hydrogen Bonds?

Back 12

The attraction for a hydrogen atom by a highly electronegative element. (Generally: F, O & N)

The strongest of the intermolecular forces.

Front 13

Dipole-Dipole Interactions?

Back 13

The attraction of one dipole on one molecule for the dipole of another molecule.

Dipole: created when an electron pair is shared unequally in a CB between two atoms or elements. This gives a + and a - side to the molecule, which attract the opposite (+ to -). Weak intermolecular force.

Front 14

Dispersion Forces?

Back 14

(aka: London dispersion forces) Weakest of all intermolecular forces. Electrons within an element or compound will concentrate themselves on one side of an atom, causing a temporary dipole.