Significant Figures (Definition)

The digits in a measured or calculated quantity that are known with certainty plus one final digit that is uncertain.

Significant Figures in Multiplication/Division

When multiplying or dividing, the result should have the same number of significant figures as the factor with the fewest sig figs.

Significant Figures in Addition/Subtraction

When adding/subtracting, align decimals and round the result to the same number of decimal places as the addend with the fewest decimal places (not sig figs).

Scientific Notation (Definition)

A way to write very large or small numbers: . It clarifies significant figures (e.g., 5.829×10⁵ has four sig figs if written that way).

Significant Figure Rules

nonzero digits are always significant; zeros between nonzero digits are significant; leading zeros are NOT significant; trailing zeros are significant only if there's a decimal point.

Temperature conversions

Formulas: °𝐹=(°𝐶×9/5)+32 °F=(°C×9/5)+32. °𝐶=(°𝐹−32)×5/9 °C=(°F−32)×5/9. 𝐾=°𝐶+273.15 K=°C+273.15.

Mass/Volume. Gases have much lower densities than solids because gas particles are far apar

identity of substance stays the same (phase changes, cutting, dissolving if no reaction)

composition changes and new substances form (tarnishing, burning, souring).

independent of sample size (density, color, melting point).

depends on sample size (mass, volume, total energy).

observed without changing chemical identity (melting point).

observed when substance undergoes chemical change (flammability, reactivity with acid).

A systematic way to convert units by multiplying by conversion factors equal to 1 (e.g., 1 ft = 12 in; 1 in = 2.54 cm). Keep track of units and cancel them algebraically.

Covalent (molecular) compounds

between nonmetals (e.g., N₂O₅).

between metals and nonmetals (e.g., SrI₂).

Binary acids (H + nonmetal, aqueous)

hydro- + root + -ic acid (e.g., HCl(aq) = hydrochloric acid)

if polyatomic ion ends in -ate → acid name ends in -ic (e.g., sulfate → sulfuric acid); if ends in -ite → ends in -ous (e.g., sulfite → sulfurous acid). So H₂SO₃(aq) = sulfurous acid.

mass of 1 mole of a substance; sum of atomic masses (from periodic table) of all atoms in formula.

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Chem Final

Question	Answer
Significant Figures (Definition)	The digits in a measured or calculated quantity that are known with certainty plus one final digit that is uncertain.
Significant Figures in Multiplication/Division	When multiplying or dividing, the result should have the same number of significant figures as the factor with the fewest sig figs.
Significant Figures in Addition/Subtraction	When adding/subtracting, align decimals and round the result to the same number of decimal places as the addend with the fewest decimal places (not sig figs).
Scientific Notation (Definition)	A way to write very large or small numbers: . It clarifies significant figures (e.g., 5.829×10⁵ has four sig figs if written that way).
Significant Figure Rules	nonzero digits are always significant; zeros between nonzero digits are significant; leading zeros are NOT significant; trailing zeros are significant only if there's a decimal point.
Temperature conversions	Formulas: °𝐹=(°𝐶×9/5)+32 °F=(°C×9/5)+32. °𝐶=(°𝐹−32)×5/9 °C=(°F−32)×5/9. 𝐾=°𝐶+273.15 K=°C+273.15.
Density	Mass/Volume. Gases have much lower densities than solids because gas particles are far apar
Physical change	identity of substance stays the same (phase changes, cutting, dissolving if no reaction)
Chemical change	composition changes and new substances form (tarnishing, burning, souring).
Intensive property	independent of sample size (density, color, melting point).
Extensive property	depends on sample size (mass, volume, total energy).
Physical property	observed without changing chemical identity (melting point).
Chemical property	observed when substance undergoes chemical change (flammability, reactivity with acid).
Dimensional analysis	A systematic way to convert units by multiplying by conversion factors equal to 1 (e.g., 1 ft = 12 in; 1 in = 2.54 cm). Keep track of units and cancel them algebraically.
Covalent (molecular) compounds	between nonmetals (e.g., N₂O₅).
Ionic compounds	between metals and nonmetals (e.g., SrI₂).
cation (positive)	Loss of electrons
anion (negative)	Gain of electrons
Binary acids (H + nonmetal, aqueous)	hydro- + root + -ic acid (e.g., HCl(aq) = hydrochloric acid)
Oxyacids	if polyatomic ion ends in -ate → acid name ends in -ic (e.g., sulfate → sulfuric acid); if ends in -ite → ends in -ous (e.g., sulfite → sulfurous acid). So H₂SO₃(aq) = sulfurous acid.
Molar mass (g/mol)	mass of 1 mole of a substance; sum of atomic masses (from periodic table) of all atoms in formula.

Created by: user-2010161

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