3A2 Systematic Naming and Formulas Flashcards

Identify chemical formulas and name simple inorganic compounds, acids, bases, salts, and hydrates.

1
Q

What is the naming convention for covalent compounds?

A
  • Use prefixes for quantity.
  • Change the ending of the second element to ‘ide’.

Example: Carbon dioxide (CO₂).

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2
Q

What is a hydrate?

A

A compound that contains water molecules within its crystal structure.

Hydrates often lose water when heated.

Hydrated compounds are often crystalline.

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3
Q

List two examples of hydrates.

A
  1. Gypsum (CaSO₄·2H₂O)
  2. Epsom salt (MgSO₄·7H₂O)

These compounds contain water in their crystalline structure.

Epsom salts are used in baths to relieve sore muscles.

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4
Q

State one property of hydrates.

A

They often dissolve in water to release their water of hydration.

This is a distinguishing characteristic of hydrates.

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5
Q

How is the formula of a hydrate determined experimentally?

A

By measuring mass before and after heating to find the water content.

This helps determine the mass of water removed.

Mass of water = Mass of hydrate - Mass of anhydrate.

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6
Q

True or False:

Anhydrous compounds are always less stable than hydrates.

A

False

Stability depends on the specific compound and environmental conditions.

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7
Q

Define:

anhydrate

A

A hydrate with the water removed.

Anhydrates are used as drying agents.

Anhydrates are formed when hydrates are heated.

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8
Q

How can a hydrate be converted to an anhydrous compound?

A

By heating the hydrate to remove water molecules.

This process is called dehydration.

An anhydrous compound does not contain water in its structure.

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9
Q

What is the naming convention for hydrates?

A
  • Name the compound.
  • Add a prefix indicating the number of water molecules.
  • Add the word ‘hydrate’.

Example: CuSO₄·5H₂O is copper (II) sulfate pentahydrate.

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10
Q

Which prefix is used for a hydrate with seven water molecules?

A

hepta-

Example: MgSO₄·7H₂O is magnesium sulfate heptahydrate.

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11
Q

What is a binary ionic compound?

A

A compound consisting of two elements: one cation and one anion.

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12
Q

List five differences between covalent and ionic compounds.

A
  1. Electrons: Shared in covalent but donated in ionic.
  2. Melting and Boiling Point: Low in covalent but high in ionic.
  3. Conduction: Poor in covalent but good in ionic.
  4. Solubility: Poor in covalent but high in ionic.
  5. Brittleness: Covalent are flexible while ionic are brittle.

These differences lead to distinct physical properties.

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13
Q

How are binary ionic compounds named?

A

With the cation first, then the anion.

Anions often end in “-ide,” “-ate,” or “-ite.”

Example: sodium chloride (NaCl).

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14
Q

Define:

polyatomic ion

A

A charged particle composed of two or more atoms covalently bonded.

Examples include sulfate (SO₄²⁻) and ammonium (NH₄⁺).

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15
Q

How do you name a transition metal in an ionic compound?

A

By using Roman numerals to indicate its oxidation state.

Example: FeCl₂ is iron (II) chloride.

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16
Q

List two examples of ionic compounds with transition metals.

A
  1. Copper (II) sulfate (CuSO₄)
  2. Iron (III) oxide (Fe₂O₃)

Transition metals often have multiple oxidation states.

17
Q

True or False:

All ionic compounds are binary.

A

False

Some ionic compounds, like calcium carbonate (CaCO₃), contain polyatomic ions.

18
Q

What is the charge of a sulfate ion?

A

-2

Sulfate’s chemical formula is SO₄²⁻.

19
Q

Define:

oxidation state

A

The charge of an atom in a compound if all bonds were ionic.

Also known as oxidation number.

20
Q

How do you write the formula for magnesium nitrate?

A

Mg(NO₃)₂

Magnesium has a +2 charge, nitrate has a -1 charge.

21
Q

Fill in the blank:

_____ chloride is the name for FeCl₃.

A

Iron(III)

The Roman numeral indicates the iron’s +3 oxidation state.

22
Q

How are acids named based on anion endings?

A
  • -ide becomes hydro -ic acid
  • -ate becomes -ic acid
  • -ite becomes -ous acid

Example:

  • HCl is hydrochloric acid
  • H₂SO₄ is sulphuric acid
  • HNO₂ is nitrous acid
23
Q

What is the naming convention for hydroxide bases?

A

The metal cation is followed by hydroxide.

Example: KOH is potassium hydroxide.

24
Q

What is an example of a strong acid?

A

Hydrochloric acid

(HCl)

Strong acids completely ionize in water.

25
Q

What is an example of a strong base?

A

Sodium hydroxide

(NaOH)

Strong bases dissociate completely in water.