Compounds, Formulae, and Equations Flashcards

Comprehensive practice flashcards covering ionic charges, polyatomic ions, formula writing, diatomic elements, and balanced chemical equations with state symbols.

How is the ionic charge of an element predicted using the periodic table?

Group 1 metals have a charge of $1+$, Group 2 metals have $2+$, and Group 3 metals have $3+$. For non-metals, Group 5 can be $3-$, Group 6 is often $2-$, and Group 7 is often $1-$. All uncombined elements are neutral.

When writing the charge of an ion, where should the number be placed relative to the sign?

The number comes before the sign (e.g., $2+$ or $3-$).

What are the formulae and charges for the ions Nitrate, Carbonate, and Sulfate?

Nitrate (V) is $NO_3^-$, Carbonate is $CO_3^{2-}$, and Sulfate (VI) is $SO_4^{2-}$.

What are the symbols and charges for Hydroxide, Ammonium, Zinc, and Silver ions?

Hydroxide is $OH^-$, Ammonium is $NH_4^+$, Zinc is $Zn^{2+}$, and Silver is $Ag^+$.

What are the formulae for the specialized ions Nitrite, Sulfite, and Hydrogencarbonate?

Nitrite (Nitrate III) is $NO_2^-$, Sulfite (Sulfate IV) is $SO_3^{2-}$, and Hydrogencarbonate is $HCO_3^-$.

What are the formulae for Dichromate, Manganate (VII), and Phosphate ions?

Dichromate is $Cr_2O_7^{2-}$, Manganate (VII) is $MnO_4^-$, and Phosphate is $PO_4^{3-}$.

What is the visual 'swap' method for working out the formula of magnesium nitrate?

Identify ions $Mg^{2+}$ and $(NO_3)^-$, swap the numbers to get $Mg_1(NO_3)_2$, resulting in the formula $Mg(NO_3)_2$.

What is the correct formula for Silver Sulfate?

$$Ag_2(SO_4)$$

List the seven diatomic elements that must be written with a subscript 2 in equations.

$H_2$, $N_2$, $F_2$, $O_2$, $I_2$, $Cl_2$, and $Br_2$.

What are the three mandatory steps for writing balanced symbol equations?

1. Write the word equation. 2. Write the correct symbols and formulae (accounting for diatoms). 3. Balance the number of each atom on each side.

Define the four state symbols used in A-level balanced equations.

$(s)$ for Solid, $(l)$ for Liquid, $(g)$ for Gas, and $(aq)$ for Aqueous (dissolved in water).

What are common states for elements and compounds at room temperature as mentioned in the notes?

$H_2$, $O_2$, $N_2$, and $Cl_2$ are gases; metals (with one exception) are solids; most ionic substances formed in water are aqueous; and most acids (e.g., $HCl$, $H_2SO_4$, $HNO_3$, $H_3PO_4$) are aqueous.

Write the balanced equation including state symbols for the reaction of sodium with water.

$$Na_{(s)} + 2H_2O_{(l)} \rightarrow H_{2(g)} + 2NaOH_{(aq)}$$

What reaction produces magnesium oxide according to the transcript?

The burning of magnesium: $2Mg_{(s)} + O_{2(g)} \rightarrow 2MgO_{(s)}$

What is produced when sulfur trioxide reacts with water?

Sulfuric acid ($H_2SO_4$).