Chemistry Naming and Formulas Quiz

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Questions and Answers

What is the correct name for the chemical formula N2O4?

Nitrogen tetroxide

Dinitrogen dioxide

Nitrogen oxide

Dinitrogen tetroxide (correct)

Which of the following correctly identifies a naming exception from the list provided?

NH3 is referred to as ammonia (correct)

H2O is called dihydrogen oxide

CO2 is known as carbon dioxane

CH4 is named carbon tetrahydride

When converting the name 'silicon dioxide' to its chemical formula, what is the correct formula?

SiO2 (correct)

Si2O2

Si2O

SiO

Which of the following compounds requires the use of the prefix 'tri-' in its name?

N2O3 Signup and view all the answers

What is the common name for the chemical formula H2SO4?

Sulfuric acid Signup and view all the answers

What should you do if a polyatomic ion has a charge greater than +1 or -1 when writing an ionic formula?

Bracket the polyatomic ion. Signup and view all the answers

When naming ionic compounds, what is the correct order of components in the name?

Cation first, then anion. Signup and view all the answers

Which suffix is associated with a compound that contains only two types of atoms?

-ide Signup and view all the answers

What is the chemical formula for the compound formed by calcium and chlorine?

CaCl2 Signup and view all the answers

Which of the following should be used to represent a formula with a polyatomic ion?

[SO4]2- Signup and view all the answers

If both the cation and anion have equal numerically charged values, what must be done to the charges in the formula?

Cancel out the charges. Signup and view all the answers

Which of the following represents a common polyatomic ion?

OH- Signup and view all the answers

In the compound formed by iron(II) and phosphate, what is the proper formula?

Fe2(PO4)3 Signup and view all the answers

Which of the following correctly describes a compound?

A substance formed when two or more chemical elements are chemically bonded together. Signup and view all the answers

When writing the formula for the ionic compound formed from aluminum and oxygen, which of the following steps is correct?

Make the magnitude of charges become the subscript for the respective ions. Signup and view all the answers

In an ionic compound, what is the relationship between the total positive charge from cations and the total negative charge from anions?

The total positive charge must equal the total negative charge. Signup and view all the answers

What do subscripts in a chemical formula represent?

The number of atoms of the preceding element in the compound. Signup and view all the answers

Which of the following correctly represents a polyatomic ion?

SO4^2− Signup and view all the answers

What is the purpose of utilizing parentheses in chemical formulas?

To group polyatomic ions in a larger compound. Signup and view all the answers

When balancing the chemical equation for an ionic reaction, what should be identified and removed?

Spectator ions that do not participate in the reaction. Signup and view all the answers

Which of the following best defines 'water of crystallization'?

Water that is chemically bonded in a crystalline structure. Signup and view all the answers

Study Notes

Chemical Formulas and Equations

Chemical formulas represent the proportions of atoms in a compound or molecule.
Chemical formulas use symbols for elements and numbers to indicate the count of each atom.
Parentheses, brackets, dashes, dots, plus (+), and minus (-) signs sometimes accompany these symbols and numbers.

Learning Goals/Objectives

Review monoatomic and polyatomic radicals (tables and formula writing)
Understand parts of a chemical equation
Understand types of chemical equations
Convert word equations to chemical equations
Convert chemical equations to word equations
Balance chemical equations
Memorize solubility rules
Write ionic/precipitation reactions
Balance ionic reactions
Define, identify, and delete spectator ions
Write net ionic reactions

Compounds, Elements, and Atoms

A compound is formed when two or more elements are chemically bonded. Example: Water (hydrogen and oxygen).
An element is a substance whose atoms all have the same number of protons (same atomic number).
An atom is the smallest unit of an element, comprised of a nucleus and orbiting electrons

Parts of a Chemical Formula

Coefficient: A number placed before a formula, indicating the molecule(s) number.
Element: A symbol representing an element (e.g., Ca)
Parenthesis: Used to group multiple atoms
Subscript: A number placed after an element symbol, indicating the number of atoms.

Water of Crystallization

A dot in a chemical formula represents weak bonds formed by water to the compound.
This weak bonding is called water of crystallization.
Heating breaks these bonds, releasing water as moisture/steam.

Writing Formulas for Ionic Compounds

Ionic compounds are comprised of positive and negative ions.
Metal cation and nonmetal anion combination
The sum of cation charges equals the sum of anion charges.
Subscripts are determined from the magnitude of the charges.

Steps for Writing Ionic Formulas

1. Write the metal symbol/charge followed by the nonmetal symbol/charge
1. Exchange the magnitudes of the charges to become subscripts (switch values).
1. If a polyatomic anion/cation has a charge greater than +/-1, enclose it in parentheses and use the magnitude of the charge on the other ion as the subscript.
1. Simplify numerical subscripts to give the smallest whole-number ratio.
1. Verify the sum of the charges are equal in the compound.

Naming Ionic Compounds

The name consists of the cation (metal) name followed by the anion (non-metal) name ending in -ide.

Use of Suffixes in Ionic Compounds

-ide: two elements present (example: lead oxide (PbO))
-ate: three or more elements present, with O as one element (example: calcium carbonate (CaCO3))
Bi-: used in names to indicate the presence of 2 as a number within the molecule (example: nitrogen dioxide)(CO2)

Rules Continued

Switch charges.
Bracket polyatomic ions with a charge greater than +1/-1
Cancel out charges with matching numerical magnitude.
Write the compound name without charges.

Types of Chemical Equations

Synthesis: Two or more reactants form a single product (example: 2H2 + O2 → 2H2O).
Decomposition: A single reactant breaks down into two or more products (example: 2HgO → 2Hg + O2).
Single Replacement: One element replaces another element in a compound (example: Zn + 2HCl → ZnCl2 + H2).
Double Replacement: The ions of two compounds exchange places in a reaction (example: AgNO3 + NaCl → AgCl + NaNO3).

Chemical Change vs. Physical Change

A chemical change results from a chemical reaction, changing the substance's chemical identity.
A physical change results from a physical change without changing the substance's chemical identity.

What is a Chemical Reaction?

Reactants change chemically to form new products.
The equation indicates the reactants and products formed.
State symbols (s, l, g, aq) identify whether a substance is a solid, liquid, gas, or dissolved in water (aqueous).

Definition of a Chemical Equation

A chemical equation describes a chemical reaction symbolically.
Reactants are on the left side, products on the right separated by an arrow.

Parts of a Chemical Equation

Reactants and products: the elements/compounds undergoing and resulting from the reaction respectively.
Coefficients: the numbers before the elements/compounds that balance the number of atoms on each side of the reaction.
Subscripts: the numbers after the elements indicating the number of atoms for each element.
State symbols (s, l, g, aq): physical states (solid, liquid, gas, aqueous solution).

Conditions in Chemical Reactions

Specific temperatures, pressures, and catalysts can be shown in the reaction to specify conditions necessary for the reaction to happen

Understanding it Better

Law of conservation of mass: matter cannot be created nor destroyed.
Mass of reactants = mass of products

Converting Chemical Equations to Word Equations

Translate the chemical formulas into compound names.
Insert appropriate words to form complete sentences stating reactants forming products.

Solubility Rules

Rules for determining the state of a substance in a reaction.
Metals (typically solid) except mercury (liquid).
Diatomic nonmetals (always gases except I2, solid; Br2, liquid).
Acids (always aqueous).
Solubility is reviewed using a solubility table (when necessary for salts and bases, which are often aqueous if soluble in water)

Ionic Equations

Represents ions participating in a reaction.
Spectator ions are those that don't participate in the reaction and are omitted from the net ionic equation.

Steps for Writing Balanced Ionic Equations

Write the balanced molecular equation.
Identify the states of reactants and products.
Dissociate all aqueous solutions into their ionic components.
Cancel spectator ions (ions that appear on both sides of the equation).
Write the net ionic equation (only showing the ions that react).

Characteristics of a Balanced Ionic Equation

Numbers of atoms, overall charge on both sides of the equation (are both zero).

Covalent Compounds

Compounds where atoms share electrons to achieve a more stable electron configuration
Covalent compounds are formed by atoms that aren't metals.
Carbon can form 4 covalent bonds.
The formula represents the number of atoms of each element in one molecule.
Use prefixes in the name to show the number of atoms (e.g., carbon dioxide CO2)

Prefix Table

Useful for naming covalent compounds (e.g mono, di, tri...).

Writing Formulas for Covalent Compounds

Determine the number of atoms of each element.
Write the chemical formula with the symbol for the central atom first.
Insert subscripts for elements after.
Use prefixes from the prefix chart to name the covalent compound using the appropriate prefix followed by the elements (e.g. carbon dioxide CO2).

Popular Acids and Bases

Memorize their formulas and names.
Some have special names like acids and bases.

Diatomic Molecules

Molecules containing two atoms of the same element.
Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), Bromine (Br2), Iodine (I2).

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Description

Test your knowledge of chemical nomenclature and formula writing with this quiz. From identifying naming exceptions to naming ionic compounds, challenge yourself with a variety of questions. Perfect for chemistry students looking to reinforce their understanding of chemical formulas and naming conventions.