Chemistry

Yes. I'd simplify it even more so it's easier to memorize while still covering the important concepts your teacher is likely to ask. I'd also remove extra details that are unlikely to appear on a Grade 11 quiz.

🧪 GENERAL CHEMISTRY REVIEW (Knowt Flashcard Format)TOPIC 1: Physical Quantities & Measurement ConversionsPhysical Quantity

A measurable property with a number and a unit.

Examples ::
Length, Mass, Time, Temperature, Volume, Area

System of Measurement

A standard way of measuring physical quantities.

Main Systems ::

SI (International System) – used by most countries

Metric System – uses meter, kilogram, liter

US Customary System – uses inch, foot, pound, gallon

SI Base Units

Length :: meter (m)

Mass :: kilogram (kg)

Time :: second (s)

Temperature :: kelvin (K)

Electric Current :: ampere (A)

Amount of Substance :: mole (mol)

Luminous Intensity :: candela (cd)

Common Derived Units

Area :: square meter (m²)

Volume :: cubic meter (m³)

Density :: g/cm³ or kg/m³

Speed :: m/s

Acceleration :: m/s²

Force :: Newton (N)

Metric Prefixes

kilo (k) = 1000

hecto (h) = 100

deca (da) = 10

Base = m, g, L

deci (d) = 0.1

centi (c) = 0.01

milli (m) = 0.001

micro (μ) = 0.000001

nano (n) = 0.000000001

Basic Metric Conversions ⭐

1 km = 1000 m

1 m = 100 cm

1 cm = 10 mm

1 kg = 1000 g

1 g = 1000 mg

1 L = 1000 mL

1 mL = 1 cm³

1 min = 60 s

1 hr = 60 min

1 day = 24 hr

Common US to Metric Conversions

1 inch = 2.54 cm

1 foot = 12 inches

1 yard = 0.914 m

1 mile = 1.609 km

1 pound = 0.453 kg

1 ounce = 28.35 g

1 gallon = 3.785 L

Sample Conversions

2.5 kg = ? g :: 2500 g

300 cm = ? m :: 3 m

750 mL = ? L :: 0.75 L

TOPIC 2: Scientific Notation

Scientific Notation ::
Writing very large or very small numbers using powers of 10.

Format ::

a × 10ⁿ

Coefficient ::

Must be between 1 and 10

Positive exponent ::

Large numbers

Negative exponent ::

Small numbers

4500 :: 4.5 × 10³

0.00045 :: 4.5 × 10⁻⁴

Multiply ::

Multiply coefficients, add exponents.

Divide ::

Divide coefficients, subtract exponents.

TOPIC 3: Accuracy & Precision

Accuracy ::

Close to the accepted value.

Precision ::

Measurements are close to each other.

Accurate but not Precise ::

Correct but scattered.

Precise but not Accurate ::

Close together but incorrect.

Accurate and Precise ::

Correct and consistent.

TOPIC 4: Density & Error

Density ::

Amount of mass in a given volume.

Formula ::

Density = Mass ÷ Volume

D = m/V

Mass ::

m = DV

Volume ::

V = m/D

Density of Water ::

1.0 g/mL

Object with density less than water ::

Floats

Object with density greater than water ::

Sinks

Types of Error

Random Error ::

Measurements vary by chance.

Systematic Error ::

Same error every time because of faulty equipment.

Human Error ::

Mistakes made by the person.

Percent Error

Formula ::

|Experimental − Accepted| ÷ Accepted × 100%

Sample ::

Mass = 20 g

Volume = 5 cm³

Density = 4 g/cm³

TOPIC 5: History of the Periodic Table

Johann Döbereiner ::

Proposed Triads

John Newlands ::

Proposed Law of Octaves

Dmitri Mendeleev ::

Father of the Periodic Table

Arranged elements by atomic mass

Predicted undiscovered elements

Henry Moseley ::

Arranged elements by atomic number

Proposed the Modern Periodic Law

Modern Periodic Law ::

Properties of elements repeat according to increasing atomic number.

TOPIC 6: Details of the Periodic Table

Period ::

Horizontal row

Group (Family) ::

Vertical column

Periods ::

Groups ::

Atomic Number ::

Number of protons

Mass Number ::

Protons + Neutrons

Neutral Atom ::

Protons = Electrons

Ion ::

Charged atom

Cation ::

Positive ion

Anion ::

Negative ion

Valence Electrons ::

Electrons in the outermost shell

Important Families

Group 1 ::

Alkali Metals

Group 2 ::

Alkaline Earth Metals

Groups 3–12 ::

Transition Metals

Group 17 ::

Halogens

Group 18 ::

Noble Gases

TOPIC 7: Periodic Trends ⭐⭐⭐Atomic Radius

Distance from the nucleus to the outermost electron.

Trend ::

⬇ Down a group = Increases

➡ Across a period = Decreases

Ionization Energy

Energy needed to remove an electron.

Trend ::

⬇ Down = Decreases

➡ Across = Increases

Electronegativity

Ability to attract electrons.

Trend ::

⬇ Down = Decreases

➡ Across = Increases

Highest ::

Fluorine (F)

Electron Affinity

Ability to gain electrons.

Trend ::

⬇ Down = Decreases

➡ Across = Generally Increases

Metallic Character

Ability to lose electrons.

Trend ::

⬇ Down = Increases

➡ Across = Decreases

Reactivity

Metals ::

Increase down Group 1

Nonmetals ::

Increase up Group 17

⭐ QUIZ MUST-KNOW

Father of the Periodic Table :: Dmitri Mendeleev

Modern Periodic Law :: Henry Moseley

Triads :: Johann Döbereiner

Law of Octaves :: John Newlands

Atomic Number :: Number of protons

Mass Number :: Protons + Neutrons

Density Formula :: D = m/V

Density Triangle ::

     M
   D   V

Accuracy :: Correct result

Precision :: Consistent result

Atomic Radius ::

⬇ Increase

➡ Decrease

Ionization Energy ::

⬇ Decrease

➡ Increase

Electronegativity ::

⬇ Decrease

➡ Increase

Metallic Character ::

⬇ Increase

➡ Decrease

Most Electronegative Element :: Fluorine (F)

Highest Ionization Energy :: Helium (He)

Least Reactive Elements :: Noble Gases (Group 18)

📌 Memory Trick for Trends

Atomic Radius: ⬇⬅ (gets bigger going down and to the left)

Ionization Energy & Electronegativity: ⬆➡ (get stronger going up and to the right)

This version focuses on the concepts, definitions, formulas, scientists, and trend directions that are most commonly tested while staying short enough to review quickly before a long quiz.