Chemistry Chapter 10 Flashcards

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Questions and Answers

What is atomic mass?

The sum of the atomic weights of atoms in a molecule

The smallest whole number ratio of the atoms in a compound

The SI unit used to measure amount of substance

The number of grams of an element that is naturally equal to the atomic mass of the element in amu (correct)

What is formula mass?

The sum of the atomic weights of atoms in a molecule

What is a mole?

The SI unit used to measure amount of substance

What is an empirical formula?

The smallest whole number ratio of the atoms in a compound Signup and view all the answers

What does STP stand for?

Standard Temperature and Pressure Signup and view all the answers

What is molar mass?

The mass of a mole of any element or compound Signup and view all the answers

What is molar volume?

The volume occupied by a mole of any gas at STP Signup and view all the answers

What is Avogadro's number?

6.02 x 10^23 Signup and view all the answers

What is molecular mass?

Sum of atomic masses of all the atoms in a molecule Signup and view all the answers

What is percent composition?

The percent by mass of each element in a compound Signup and view all the answers

What are the representative particles?

Atoms (Al), Molecules (H2O), Ions (NO3-) Signup and view all the answers

What are the diatomic elements?

Hydrogen, Nitrogen, Oxygen, Bromine, Fluorine, Chlorine, Iodine Signup and view all the answers

What is the value of Avogadro's number?

6.02 x 10^23 Signup and view all the answers

What is the relationship of Avogadro's number?

1 mol = Avogadro's number Signup and view all the answers

What is the molar volume of a gas at STP?

22.4 L Signup and view all the answers

What is the value of ST?

0 degrees Celsius (273 K) Signup and view all the answers

What is the value of SP?

101.3 kPa Signup and view all the answers

Can the empirical formula of C6H12O6 be simplified?

True Signup and view all the answers

What are three ways quantities can be measured?

Mass, Volume, Count Signup and view all the answers

Determine moles of an atom: Atom's subscript x number of moles of molecule (0.2 mol H2O = 0.4 x 0.2 = _____ mol)

0.4 Signup and view all the answers

Determine the total number of atoms: Number of atoms in formula x mol of substance x Avogadro's number (0.7 mol C6H6 = 0.7(12)(6.02 x 10^23)) = _____

0.7 * 12 * 6.02 x 10^23 Signup and view all the answers

How do you calculate gmm?

Add atomic masses Signup and view all the answers

What is molar mass conversion?

Grams given / atomic masses added up. Signup and view all the answers

What is the density of gases at STP?

G-fwt of gas / 22.4 L = g/L Signup and view all the answers

How to find mole of gas from volume at STP?

Volume given (L) / 22.4 L = mol Signup and view all the answers

How to find gas volumes from moles at STP?

Mole given x 22.4 L = L Signup and view all the answers

What is the formula for percent composition?

Mass of element in compound / g-fwt of compound x 100 Signup and view all the answers

What is the molecular formula relationship?

g-mm = (empirical)x Signup and view all the answers

Study Notes

Atomic Concepts

Atomic mass: Measured in grams, equivalent to the element's atomic mass in amu.
Mole: SI unit for amount of substance, crucial in determining quantities in chemical reactions.
Molar mass: Mass of one mole of an element or compound, vital for stoichiometric calculations.
Molecular mass: Total of atomic masses in a molecule, essential for understanding molecular weight.

Formulas and Ratios

Empirical formula: Represents the simplest whole-number ratio of elements in a compound, showing relative proportions.
Molecular formula: Shows the actual number of atoms of each element in a molecule, derived from empirical formula multiplied by a whole number.
Percent composition: Calculation of the percentage by mass of each element in the compound, key for determining formula stoichiometry.

Gas Laws and Concepts

STP (Standard Temperature and Pressure): Defined as 0 degrees Celsius (273 K) and 1 atm (101.3 kPa), important for gas calculations.
Molar volume of gas at STP: Occupies 22.4 L, essential for converting between volume and moles of gas.
Density of gases at STP: Density calculated as grams of substance per 22.4 L, useful for gas property assessments.

Key Constants

Avogadro's number: 6.02 x 10^23, the number of representative particles in one mole, fundamental in molecular counting.

Measurement Techniques

Representative particles: May include atoms (e.g., Al), molecules (e.g., H₂O), or ions (e.g., NO₃⁻), depending on the substance.
Three ways to measure quantities: Mass, volume, and count, crucial for quantifying substances in chemistry.

Calculation Methods

Molar mass conversion: Calculate the number of moles by dividing grams by molar mass or vice versa, vital for stoichiometric problem-solving.
Determining total number of atoms: Multiply the number of atoms in a formula by the number of moles and Avogadro's number.
Calculating grams per mole (gmm): Summation of atomic masses to find the molecular weight of compounds.

Special Cases

Diatomic elements: Hydrogen, Nitrogen, Oxygen, Bromine, Fluorine, Chlorine, and Iodine exist naturally as molecules composed of two atoms.
Empirical vs. molecular formula determination: Example provided: C₆H₁₂O₆ can be simplified to C₁H₂O, showcasing the difference between empirical and molecular representations.

Practical Applications

Conversion between moles and gas volumes at STP: Calculate moles using volume divided by 22.4 L or vice versa to understand gas behavior in reactions.
Percent composition formula: Key for analyzing the makeup of compounds (mass of element in compound divided by the formula weight of compound, multiplied by 100).

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Description

Explore key concepts from Chapter 10 of Chemistry with these flashcards. Each term is defined to help reinforce your understanding of atomic mass, formula mass, moles, and empirical formulas. Prepare to ace your chemistry studies!