Chemistry Fundamentals and Mnemonic Review

Vocabulary practice flashcards covering basic physical quantities, SI prefixes, unit conversions, ion charges, functional groups, polyatomic oxyanions, solubility mnemonics, strong acids and bases, and STP properties.

Five Fundamental Quantities

Mass, length, time, temperature, and number of particles.

$$1\,\text{cm}^3$$

Equivalent to a volume of $1\,\text{mL}$.

Tera ($\text{T}$)

Metric prefix representing $10^{12}$.

Giga ($\text{G}$)

Metric prefix representing $10^9$.

Mega ($\text{M}$)

Metric prefix representing $10^6$.

Kilo ($\text{k}$)

Metric prefix representing $10^3$.

Deci ($\text{d}$)

Metric prefix representing $10^{-1}$.

Centi ($\text{c}$)

Metric prefix representing $10^{-2}$.

Milli ($\text{m}$)

Metric prefix representing $10^{-3}$.

Micro ($\mu$)

Metric prefix representing $10^{-6}$.

Nano ($\text{n}$)

Metric prefix representing $10^{-9}$.

Pico ($\text{p}$)

Metric prefix representing $10^{-12}$.

Fahrenheit to Celsius Conversion Formula

$$^\circ\text{C} = (^\circ\text{F} - 32) \times \frac{5}{9}$$

Celsius to Fahrenheit Conversion Formula

$$^\circ\text{F} = (^\circ\text{C} \times \frac{9}{5}) + 32$$

Celsius to Kelvin Conversion Formula

$$\text{K} = ^\circ\text{C} + 273.15$$

Kelvin to Celsius Conversion Formula

$$^\circ\text{C} = \text{K} - 273.15$$

Group 1 Alkali Metals Ion Charge

Form ions with a charge of $1+$.

Group 2 Alkaline Earth Metals Ion Charge

Form ions with a charge of $2+$.

Group 17 Halogens Ion Charge

Form ions with a charge of $1-$.

Group 18 Noble Gases

Very stable/unreactive elements that generally do not form ions.

Seven Diatomic Elements

$\text{Br}_2$, $\text{I}_2$, $\text{N}_2$, $\text{Cl}_2$, $\text{H}_2$, $\text{O}_2$, and $\text{F}_2$.

BrINClHOF

Mnemonic used to remember the 7 diatomic elements ($\text{Br}_2$, $\text{I}_2$, $\text{N}_2$, $\text{Cl}_2$, $\text{H}_2$, $\text{O}_2$, $\text{F}_2$).

Silver Ion Charge

$\text{Ag}$ forms $\text{Ag}^+$.

Zinc Ion Charge

$\text{Zn}$ forms $\text{Zn}^{2+}$.

Cadmium Ion Charge

$\text{Cd}$ forms $\text{Cd}^{2+}$.

Aluminum Ion Charge

$\text{Al}$ forms $\text{Al}^{3+}$.

Gallium Ion Charge

$\text{Ga}$ forms $\text{Ga}^{3+}$.

Indium Ion Charge

$\text{In}$ forms $\text{In}^{3+}$.

1-2-3 Stair-Step Rule

Rule for specific metal charges: $\text{Ag} = 1+$; $\text{Zn}$ and $\text{Cd} = 2+$; $\text{Al}$, $\text{Ga}$, and $\text{In} = 3+$.

Alkene

Functional group containing a carbon-carbon double bond ($\text{C}=\text{C}$).

Alkyne

Functional group containing a carbon-carbon triple bond structure (listed as $\text{C}=\text{C}$ in notes).

Alcohol

Functional group containing $\text{R-OH}$.

Ether

Functional group containing $\text{R-O-R'}$.

Aldehyde

Functional group containing $\text{R-CHO}$.

Ketone

Functional group containing $\text{R-CO-R'}$.

Carboxylic Acid

Functional group containing $\text{R-COOH}$.

Ester

Functional group containing $\text{R-COO-R'}$.

Amine

Functional group containing nitrogen bonded to carbon/hydrogen with no adjacent $\text{C}=\text{O}$.

Amide

Functional group containing $\text{R-CONH}_2$ or related $\text{C}(=\text{O})-\text{N}$ structure.

Ammonium

Polyatomic ion with formula $\text{NH}_4^+$.

Cyanide

Polyatomic ion with formula $\text{CN}^-$.

Hydroxide

Polyatomic ion with formula $\text{OH}^-$.

Acetate

Polyatomic ion with formula $\text{CH}_3\text{COO}^-$ or $\text{C}_2\text{H}_3\text{O}_2^-$.

-ate to -ite Conversion Rule

Remove 1 oxygen atom while keeping the same charge.

Nitrite

Polyatomic ion with formula $\text{NO}_2^-$.

Sulfite

Polyatomic ion with formula $\text{SO}_3^{2-}$.

hypo-…-ite Prefix/Suffix Rule

Designates an oxyanion with 2 fewer oxygen atoms than the -ate ion, keeping the same charge.

per-…-ate Prefix/Suffix Rule

Designates an oxyanion with 1 more oxygen atom than the -ate ion, keeping the same charge.

Perchlorate

Polyatomic ion with formula $\text{ClO}_4^-$.

Chlorite

Polyatomic ion with formula $\text{ClO}_2^-$.

Hypochlorite

Polyatomic ion with formula $\text{ClO}^-$.

Hydrogen Carbonate Formation

Formed by adding $\text{H}^+$ to carbonate: $\text{CO}_3^{2-} \rightarrow \text{HCO}_3^-$.

Hydrogen Phosphate Formation

Formed by adding $\text{H}^+$ to phosphate: $\text{PO}_4^{3-} \rightarrow \text{HPO}_4^{2-}$.

NAPSACHS Mnemonic

Solubility rule mnemonic representing Nitrate ($\text{NO}_3^-$), Ammonium ($\text{NH}_4^+$), Potassium ($\text{K}^+$), Sodium ($\text{Na}^+$), Acetate ($\text{CH}_3\text{COO}^-$), Chlorates ($\text{ClO}_3^-$, $\text{ClO}_4^-$), Halides ($\text{Cl}^-$, $\text{Br}^-$, $\text{I}^-$), and Sulfate ($\text{SO}_4^{2-}$).

Halide Solubility Exceptions

Halides ($\text{Cl}^-$, $\text{Br}^-$, $\text{I}^-$) are insoluble when paired with $\text{Pb}^{2+}$, $\text{Hg}_2^{2+}$, or $\text{Ag}^+$.

Sulfate Solubility Exceptions

Sulfate ($\text{SO}_4^{2-}$) is insoluble when paired with $\text{Pb}^{2+}$, $\text{Hg}_2^{2+}$, $\text{Ag}^+$, $\text{Ca}^{2+}$, $\text{Sr}^{2+}$, or $\text{Ba}^{2+}$.

Hydroxide ($\text{OH}^-$) Solubility Rules

Generally insoluble, with exceptions being all Group 1 metal ions, $\text{Ca}^{2+}$, $\text{Sr}^{2+}$, and $\text{Ba}^{2+}$.

Seven Strong Acids

$\text{HCl}$, $\text{HBr}$, $\text{HI}$, $\text{HNO}_3$, $\text{HClO}_3$, $\text{HClO}_4$, and $\text{H}_2\text{SO}_4$.

Eight Strong Bases

$\text{LiOH}$, $\text{NaOH}$, $\text{KOH}$, $\text{RbOH}$, $\text{CsOH}$, $\text{Ca(OH)}_2$, $\text{Sr(OH)}_2$, and $\text{Ba(OH)}_2$.

Standard Temperature and Pressure (STP) Conditions

Temperature of $0\,^\circ\text{C}$ ($273.15\,\text{K}$) and pressure of $1\,\text{atm}$.

Molar Volume of a Gas at STP

$22.41\,\text{L/mol}$.