Grade 11 ChemistryEvelyn Clay, Sem 1 2021-2022Ms. Papaiconomou

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Chemistry Chemistry is ultimately the study of matter including how it behaves and . Additionally in this unit we talked about how to describe properties and changes using diagrams and nomenclature, and equations.

după Ragubavan Sathurtheha

Areas of Interest

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Indigenous situation in Colombia.

după Juan Felipe Melo Vega

Special Cases

după Shela Lamug

Floating topic

A substance that turns blue litmus paper red

Ionizes in water to form [H+] ions

1-6

Can be dangerous, CO prevents oxygen transport in the body

Shared reactions

Element

=Binary compound

Non-metallic oxide

=Acid

Metallic halide

=Chlorate/bromate/iodate

Metallic oxide

=Carbonate

=Base

Representative element: closely follow periodic law

Grade 11 Chemistry Evelyn Clay, Sem 1 2021-2022 Ms. Papaiconomou

Unit 4: Solutions and Solubility

Qualitative Analysis

Used to find ion presence if a precipitate forms or not

Some ions turn flame into a different colour

Sequential chemical analysis

Some ions turn a different colour in solution

Calculations involving the solution concept

Solution Stoichiometry

Requires molar concentration equation and n=m/M equation

CiVi=CfVf

Concentration (C)

In small quantities

ppb=(Mass of solute (g)) x10^9 (Mass of solution (g))

ppm=(Mass of solute (g)) x10^6 (Mass of solution (g))

%=(Volume of solute (ml)) x100% (Volume of solution (mL))

%=(Mass of solute (g)) x100% (Mass of solution (g))

%=(Mass of solute (g)) x100% (Volume of solution (mL))

C=Amount of solute(n) Volume of solution(L)

Acids and Bases

Acid

Base

A substance that turns red litmus paper blue

Dissociates in water to form [OH-] ions

8-11

pH and [H+] concentration

pH of 7

10^-pH

-log[H+]

Solution, a mixture of at least 1 solute and solvent

Solubility

Temp vs g dissolved per 100g of H2O

Supersaturated solution

Saturated solution

Unsaturated solution

Polar dissolves polar, ionic and polar substances can be dissolved in polar

Ionic substances with + and - parts get pulled apart by polar substances

Solvent

Solute

Unit 5: Gases and Atmospheric Chemistry

Gas Stoichiometry

Stoichiometry (Unit 3)

n=v Vmolar

Vmolar=24.8L/mol

Vmolar=22.4L/mol

Gas Laws

Combined gas law

P1V1=P2V2 T1 T2

Ideal gas law

n=PV RT

Ideal gas constant: 8.31 kPaL/molK

Amonton's Law

P1=P2 T1 T2

Charle's Law

V1=V2 T1 T2

Boyle's Law

P1V1=P2V2

Pressure

760Hgmm=1atm

760torr=760Hgmm

1 atm=101.325kPa

Temperature

0k or -273 Celsius

Celsius=Kelvin-273

Kelvin=Celsius+273

Unit 1: Matter, Chemical Trends and Chemical Bonding

Atomic Theory

Energy Levels

Neils Bohr

Nucleus

Neutrons

James Chadwick

Protons

Ernst Rutherford

Alpha, Beta, Gamma Rays

Electrons

Electronegativity determines polarity

J.J. Thomson

Periodic Table

Dmitri Mendeleev

Mendeleev's periodic law: Elements arranged by increasing atomic mass

Modern periodic law: Elements arranged by increasing atomic number

Vertically, by Group

-Nuclear charge increases -Shielding effect increases -Atomic radius increases -Ionization energy decreases -Electronegativity decreases -Electron affinity decreases

More protons in nucleus means greater attraction of valence electrons

Repulsion of valence electrons by inner electrons

Horizontally, by period

-Nuclear charge increases -Shielding effect is constant -Atomic radius decreases -Ionization energy increases -Electronegativity increases -Electron affinity increses

6 Metalloids

Shiny like metals, brittle like non-metals

Staircase line

17 Non-metals

Group 17: Halogens

Group 18: Noble Gases

Unreactive due to full valence shell

95 Metals

A metal and non-metal can form an ionic compound

Mostly solid at SATP, conduct heat and electricity well

Groups 3-12: Transition Metals

Group 2: Alkaline Earth Metals

Group 1: Alkali Metals

Unit 2: Chemical Reactions

Different Types of Chemical Reactions

Balanced equation needed: # of mols of each element on one side must match other side

Double Displacement

2 reactants, forming 2 products

Each reactant has 2 elements, molecules, polyatomic ions etc.

Single Displacement

Halogen

Lone halogen replaces halogen in compound

Metal

Hydrogen gas and metal hydroxide OR ionic compound produced

Lone metal replaces metal in compound

Only occurs if lone metal is higher on activity series than metal in compound

Combustion, reactants are fuel and oxygen gas

Complete Combustion

Flame is blue or invisible

Incomplete Combustion

Flame is orange, black soot produced

Soot (solid carbon) and carbon monoxide

Products are CO2 gas, water vapour and energy

Exothermic reaction produces thermal energy

Decomposition

One product, breaking down into 2 reactants

Synthesis

2 reactants, forming 1 product

Unit 3: Quantities in Chemical Reactions

Balanced chemical equation needed for all calculations

Law of conservation of mass

The mole, n

Calculations involving the mole concept

Stoichiometry

nwant=nhave*(#of mols want) (# of mols have)

Percentage yield

%yield=(actual yield) * 100% (theoretical yield)

Amount of product actually produced

Amount of product that could be produced

Limiting and excess reagents

nproduct=nhave*(#of mols reactant) (# of mols product)

Reactant that is not used up first

Reactant that is used up in reaction

The smaller mole product #

Empirical and molecular formulas

Finding actual # of elements in a compound

Finding simplest whole # ration of atoms/ions

Percentage composition

%xtotal=(mx/mtotal)*100%