The discussed concepts encompass the mechanisms of energy transfer and the various states of matter, focusing on the roles of heat and enthalpy in phase changes. The behavior of small covalent molecules, particularly gases under different conditions, is highlighted, emphasizing their phase transitions and solubility properties.
When an acid reacts with base, it forms an ionic compound and water
Produce a precipitate or solid
Diagram
Potential Energy Diagram
Increasing KE = 0
Phase will change with melting and boiling point at this time heat is still adding in but temperature does not change so KE is constant. Change in phase does not involve change in KE
Increasing KE = +
KE only changes during the slope of the phase change diagram. At this time all of heat added isused to speed up particles
Melting Point
Boiling Point
Phase
State
Phase change diagrams
Kinetic Energy
Movement
Potential Energy
Energy is stored in bonds and inter molecular forces of attraction. During the plateau inter molecular forces of attraction are changing therefore PE changes
Stored Energy
Neutralization Reaction
Precipitation reaction
Release energy to let particals ties together and put in more energy to let it break
G
L
S
A+B = A+B+Energy
A+B → C+D ΔH= -KJ
A+B+Energy = C+D
A+B → C+D ΔH= +KJ
Exothermic Reaction
Gain energy in the environment
- ΔH
More energy is released to make the bond than required when new bond is formed
Endothermic Reaction
H is at the Reactants
Less energy in the environment
+ ΔH
More energy is required to break the bond than released when new bond is formed
A change or transfer in energy are called the Heat, or enthalpy, the symbol for enthalpy is ΔH
Energ Changes
Making Bonds/Attraction: Energy is released
Breaking Bonds/Attraction: Energy is required
Energy is measured in Joules (J) often kilo joules (KJ)
1000J = 1kj
Prediction products
Single Replacement
Occurs when an element reacts with a compound to produce an new element and compound
A+BC = B+AC
Double Replacement
Occurs two Ionic compounds reacts together
AB+CD = AD+CB
Combustion
Involving burning a substance with Oxygen
AB+O2 =CO2+H2O
Decomposition
When one reactant break down to two or more product.
AB = A+B
Synthesis
When two or more reactants combine to make one product
A+B = AB
Solubility
Low solubility = solid
Soluble = aqueous
Organic Compounds
Hydro Carbons
16+ Carbon = Solid
5-15 Carbon = Liquid
1-4 Carbon = Gas
Functional groups are mostly liquid
Ionic Compounds
Ionic compound dissolving completely in the water which forms homogeneous solution
These compounds are soluble and it will be aqueous (aq)
Many solution involve mixing, which means water is present.
Other only dissolve lightly, which forms a heterogenous mixture.
These compounds are low solubility so it will be solid (s)
When no water its solid
Small Covalent molecules
Pure NH3 is gas in room tempture
HF is also Hydrogen-Bonds, you can use it as l or g
Water is produced as a gas in combustion
Usually Gases unless its water
State changes
Phase Changes
Gas
Solid
Liquid
When a system is closed the mass of the reactants always equals the mass of products
May difficult to reverse
New State
Energy Changed (Bond form or broken)
New color/ New smell
Used to separate a mixture into pure
A phase changes
No new substance formed
Definition: Result in the formation of new substances, which have a different properties and chemical composition
Definition: Occurs when a substance changes form, does not change it chemical composition.
