Chemistry

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Chemistry by Mind Map: Chemistry

1. Bohr Models

1.1. shows the way an element is structured

1.2. easy way to have drawn model of element

2. Types of Radiation

2.1. Gamma

2.1.1. strongest type of radiaton

2.1.2. transmutation does not occur during decay

2.2. Beta

2.2.1. stronger than alpha

2.2.2. transmutation occurs during decay

2.3. Alpha

2.3.1. weakest type of radiaton

2.3.2. transmutation occurs during decay

3. Half life

3.1. the average length of time for half of the parent nuclei in a sample to decay

4. Nuclear Reactions

4.1. Fission

4.1.1. large nucleus is split into two smaller nuclei

4.1.2. total mass of the products produced is smaller than the original mass

4.2. Fussion

4.2.1. two small nuclei are joined into one nucleus

5. Collision Theory

5.1. for a reaction to occur molecules need to be moving and collide to react

5.2. factors that affect reaction rates;

5.2.1. concentration of reactants

5.2.2. surface area of reactants

5.2.3. temperature

5.2.4. catalysts

6. Reaction types

6.1. synthesis

6.1.1. two or more reactants form a compound

6.2. decompisition

6.2.1. a compound breaks into two or more products

6.3. single replacement

6.3.1. in a compound replace one element with a other one added as a reactant

6.4. double replacement

6.4.1. elements form compounds swap to form new compounds

6.5. combustion

6.5.1. a compound or element reacts with oxygen to create oxide and release energy

7. Law of Concervation of mass

7.1. mater is not created or lost in a chemical reaction

7.2. total mass of the reactants is the total mass of the products

8. Organic Compounds

8.1. hydrocarbons

8.1.1. flamable

8.1.2. most are liquid at room tempture

8.1.3. simple hydrocarbons

8.1.3.1. methane

8.1.3.2. ethane

8.1.3.3. butaine

8.1.3.4. pentane

8.1.4. contains only carbon and hydrogen

8.2. alcohols

8.2.1. good solvents

8.2.2. flamabel

8.2.3. simple alcohols

8.2.3.1. methanol

8.2.3.2. ethanol

8.2.3.3. isopropyl alcohol

9. Periodic Table

9.1. Classification of elements

9.1.1. Metals - on the left

9.1.2. Non metals - on the right

9.2. 5 Chemical familys

9.2.1. 1. Alkali Metals

9.2.2. 2. Alkaline Earth Metals

9.2.3. 3. Halogens

9.2.4. 4. Noble Gasses

9.2.5. 5. Transition Metals

9.3. Atomic Number / Mass

9.3.1. help with figuring out number of protons

10. Classifications of Acids, Bases, and Salts

10.1. Acids

10.1.1. release H+ ions in solution

10.1.2. conduct electricity

10.1.3. react with some metals to produce hydrogen gas

10.1.4. cause chemical indicators to change color

10.2. Bases

10.2.1. release OH- ions in solution

10.2.2. conduct electricity

10.2.3. do not react with metals to produce hydrogen gas

10.2.4. cause chemical indicators to change color

10.3. Salts

10.3.1. release "+" and "-" ions other than H+ and OH- in solution

10.3.2. conduct electricity

10.3.3. no effect on chemical indicators

10.3.4. do not react with metals to produce hydrogen

11. Bonding Types

11.1. Ionic Bonding

11.1.1. Ionic Compounds

11.1.1.1. strong-due to electrical attraction of opposite charges

11.1.1.2. form crystals

11.1.1.3. high melting points

11.1.1.4. very hard and brittle

11.1.1.5. conduct electricity when dissolved in water

11.1.2. Ionic Formulas

11.1.2.1. simple binary compounds

11.1.2.1.1. change ending to ide

11.1.2.1.2. no space between names

11.1.2.2. ionic compound where the first element has more than one combining capicity

11.1.2.2.1. use a roman numeral to tell the combining capicity

11.1.2.2.2. use criss-cross to find combining capicity

11.1.2.2.3. omit 1 in superscript

11.1.2.3. ionic compounds with polyatomic ions

11.1.2.3.1. do not change the ending if it is polyatomic

11.1.2.3.2. polyatomic ions are named as one

11.1.2.3.3. place bracket around a polyatomic ions

11.1.2.3.4. omit 1 in a superscript

11.1.2.3.5. use criss-cross to find superscript

11.2. Covalent Bonding

11.2.1. covalent componds

11.2.1.1. non metals share their valence electrons with other non metal to complete valence shells

11.2.1.2. form crystals

11.2.1.3. low melting and boiling points

11.2.1.4. poor conductor of electricity

11.2.2. covalent formulas

11.2.2.1. contains non metals only

11.2.2.2. use prefixes to identify the number of each element

11.2.2.3. only can omit mono foe the first element

11.2.2.4. do not crosover

11.3. Balancing equations

11.3.1. balance compounds first

11.3.2. balance one at a time

11.3.3. do not change subscripts only add subscripts

11.3.4. try to ballance O and H last if they apear more than once

11.3.5. try to balence polyatomic ions as a group