Ionic and Acid Naming Quiz

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Questions and Answers

What is the name of the compound NaCl?

Sodium Oxide

Sodium Chloride (correct)

Sodium Fluoride

Chloride Sodium

Acids derived from -ite ions end with the suffix -ic acid.

False (B)

What is the formula for Calcium Carbonate?

CaCO₃

Fe₂O₃ is named ________.

Iron(III) Oxide Signup and view all the answers

Which of the following represents a molecular compound?

N₂O₄ (C) Signup and view all the answers

What is the prefix used for 4 atoms in a molecular compound?

tetra- Signup and view all the answers

Match the following acids with their correct names:

H₂SO₄ = Sulfuric Acid HCl = Hydrochloric Acid H₂CO₃ = Carbonic Acid HNO₃ = Nitric Acid Signup and view all the answers

The charge of Silver is always represented as ______.

Ag+ Signup and view all the answers

Which of the following statements about covalent compounds is true?

They are made solely of nonmetals. (A) Signup and view all the answers

The seven diatomic elements are H₂, N₂, O₂, F₂, Cl₂, Br₂, and He₂.

False (B) Signup and view all the answers

What is the physical state of Mercury (Hg) at room temperature?

Liquid Signup and view all the answers

A molecule with a trigonal planar shape has _____ bond angles.

120° Signup and view all the answers

Match the following group of elements with their corresponding group name:

Lithium (Li) = Alkali Metals Fluorine (F) = Halogens Calcium (Ca) = Alkaline Earth Metals Neon (Ne) = Noble Gases Signup and view all the answers

Which ionic compound would have high melting points?

NaCl (A) Signup and view all the answers

Ionic bonds occur when electrons are shared between atoms.

False (B) Signup and view all the answers

What ion does Sodium (Na) typically form?

Na⁺ Signup and view all the answers

The formula for hydroxide is _____ .

OH⁻ Signup and view all the answers

Which statement is true regarding the octet rule?

Hydrogen seeks to have 2 electrons for stability. (A) Signup and view all the answers

Study Notes

Ionic Naming

Binary Compounds: Ionic compounds composed of one metal and one nonmetal.
- Naming Rule: Name the metal cation first, then the nonmetal anion with the -ide suffix.
- Example: NaCl (Sodium Chloride).
Polyatomic Ions: Ionic compounds with more than two atoms (often oxygen and another element).
- Naming Rule: Name the metal cation first, then the polyatomic anion. Polyatomic ions usually end in -ate or -ite.
- Example: Na₂SO₄ (Sodium Sulfate).
Roman Numerals for Transition Metals: Many transition metals have more than one possible charge.
- Naming Rule: Use Roman numerals in parentheses after the metal cation to indicate the charge.
- Examples: FeCl₂ (Iron(II) Chloride), Fe₂O₃ (Iron(III) Oxide).
- Exceptions: Silver (Ag⁺) and Zinc (Zn²⁺) always have a single charge.

Acid Naming

Acids Ending in -ate: Replace -ate with -ic acid.
- Example: H₂SO₄ (Sulfuric Acid).
Acids Ending in -ite: Replace -ite with -ous acid.
- Example: H₂SO₃ (Sulfurous Acid).
Acids Ending in -ide: Add "hydro-" to the beginning, replace -ide with -ic acid.
- Example: HCl (Hydrochloric Acid).

Molecular Naming

Covalent Compounds: Compounds formed by sharing electrons between nonmetals.
- Naming Rule: Use prefixes to denote the number of atoms of each element. Omit "mono-" for the first element.
- Prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-.
- Example: CO (Carbon Monoxide), N₂O₄ (Dinitrogen Tetraoxide), P₄O₁₀ (Tetraphosphorus Decoxide).

Ionic vs. Covalent Compounds

Ionic Compounds: Metal and nonmetal, high melting point, conduct electricity when molten or dissolved.
Covalent Compounds: Nonmetal and nonmetal, low melting point, generally do not conduct electricity.

Double Replacement Reactions

Double Replacement Reaction: Two ionic compounds react, ions switch partners forming new compounds.
- Example: AgNO₃ + NaCl → AgCl + NaNO₃

States of Matter

Solid: Atoms/molecules are closely packed.
Liquid: Atoms/molecules are spaced further and can move past each other.
Gas: Atoms/molecules are widely spaced and freely move.

Diatomics

Diatomic Elements: Elements that exist in nature as two-atom molecules.
- List: H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂.

Bonding and Octet Rule

Ionic Bonding: Electrons are transferred.
Covalent Bonding: Electrons are shared.
Octet Rule: Atoms tend to complete their outer electron shell with 8 electrons (except H, which wants 2 – a "duet").
Exceptions: Beryllium(Be) often has 4 electrons, Boron (B) often has 6, Phosphorus (P) often has 10, and Sulfur (S) often has 12 or more in its valence shell. Similarly, some elements in period 3 and onwards can exceed the octet rule.

Lewis Structures

Ionic Bonding: Electrons transferred forming ions.
Covalent Bonding: Electrons shared forming bonds.

Formal Charge

Formula: valence electrons - (bonds + lone pairs)
Purpose: To help determine the better Lewis structure – The structure with the fewest or smallest formal charges is preferred.

Charges of Ions

Identify the element and predict the associated ion based on its position and charge tendency. -Example; Sodium (Na⁺), Oxygen (O⁻²), Nitrogen (N⁻³).

Group Names

Group 1: Alkali Metals
Group 2: Alkaline Earth Metals
Group 17: Halogens
Group 18: Noble Gases

Reactivity and Electronegativity Trends

Reactivity Trends: Group 1 (Alkali Metals) and Group 17 (Halogens) are highly reactive.
Electronegativity: Tends to increase across a period and decrease down a group.

Polyatomic Ions

Polyatomic Ions: Groups of atoms that have a collective charge.
- Examples: Nitrate (NO₃⁻), Phosphate (PO₄³⁻), Hydroxide (OH⁻).

VSEPR Theory (Molecular Shapes)

Molecular Shapes:
- Linear: 180° (e.g., CO₂)
- Bent: <120° (e.g., H₂O)
- Trigonal Planar: 120° (e.g., BF₃)
- Tetrahedral: 109.5° (e.g., CH₄)

Dimensional Analysis

Conversions: Use conversion factors (e.g., 1 km = 1000 m, 1 g = 1000 mg, °C to K).
Examples: Convert km to meters, grams to milligrams, °C to Kelvin.

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Description

Test your knowledge on the naming conventions for ionic compounds and acids. This quiz covers binary compounds, polyatomic ions, and special rules for transition metals. Brush up on your chemistry skills and see how well you understand these essential naming rules!