Chemistry Concepts and Calculations Quiz

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Questions and Answers

Which of the following is the correct equation for energy in terms of wavelength?

  • E = hλ
  • E = λν
  • E = hc/λ (correct)
  • E = hν

Gamma rays have longer wavelengths than visible light.

False (B)

What are valence electrons?

Electrons in the outermost shell of an atom that are involved in chemical bonding.

The frequency of a wave can be calculated using the formula ___ = c/λ.

<p>ν</p> Signup and view all the answers

Match the following concepts of light with their characteristics:

<p>Infrared = Lower energy than visible light Visible light = Can be seen by the human eye Ultraviolet = Higher energy than visible light X-rays = Used in medical imaging</p> Signup and view all the answers

What is the theoretical percent composition of hydrogen in methane (CH4)?

<p>25% (D)</p> Signup and view all the answers

The empirical formula provides information on the actual number of atoms in a molecule.

<p>False (B)</p> Signup and view all the answers

What is the molar mass of caffeine if it contains 49.47 g carbon, 28.85 g nitrogen, 16.48 g oxygen, and 5.20 g hydrogen?

<p>194.19 g/mol</p> Signup and view all the answers

The density equation is given by the formula d = _______.

<p>mass/volume</p> Signup and view all the answers

Match the following compounds with their percent compositions:

<p>CH4 = 75% H, 25% C C6H12O6 = 40% C, 6.6% H, 53.3% O CO2 = 27.3% C, 72.7% O C2H8N = Various based on empirical formula</p> Signup and view all the answers

How can the molecular formula be determined from the empirical formula?

<p>By finding the ratio of molar mass to empirical mass (B)</p> Signup and view all the answers

What is the empirical formula for a compound consisting of 88.8% copper and 11.2% oxygen?

<p>CuO</p> Signup and view all the answers

What is produced when solid lithium hydroxide reacts with carbon dioxide?

<p>Solid lithium carbonate and liquid water (B)</p> Signup and view all the answers

The molar mass of magnesium is approximately 24.31 g/mol.

<p>True (A)</p> Signup and view all the answers

If the actual yield of FeCl3 is 5.22 g, what formula would you use to calculate the percent yield?

<p>% yield = (actual yield / theoretical yield) x 100%</p> Signup and view all the answers

The limiting reactant is the reactant that produces the _______ yield.

<p>smaller</p> Signup and view all the answers

Match the following substances with their formula:

<p>Lithium Hydroxide = LiOH Magnesium Oxide = MgO Carbon Dioxide = CO2 Iron(III) Chloride = FeCl3</p> Signup and view all the answers

What is the theoretical yield of Magnesium Oxide if magnesium is the limiting reactant?

<p>3.98 g (C)</p> Signup and view all the answers

For the reaction of iron with chlorine, Fe is the limiting reactant if it produces fewer moles of FeCl3 than Cl2.

<p>True (A)</p> Signup and view all the answers

How many moles of Cl2 are needed to completely react with 2.30 g of Fe?

<p>0.0344 moles</p> Signup and view all the answers

The reaction formula for the formation of magnesium oxide from magnesium and oxygen is: Mg + O2 → _______.

<p>MgO</p> Signup and view all the answers

Which of the following represents a binary acid?

<p>HF (C)</p> Signup and view all the answers

Copper(II) sulfate is represented by the formula CuSO4.

<p>True (A)</p> Signup and view all the answers

What is the formula for sulfuric acid?

<p>H2SO4</p> Signup and view all the answers

Ni3(PO4)2 is known as nickel(II) ______.

<p>phosphate</p> Signup and view all the answers

Which compound is an oxyacid?

<p>CH₃COOH (A)</p> Signup and view all the answers

Match the following ionic compounds with their formulas:

<p>Sodium chloride = NaCl Calcium bromide = CaBr2 Magnesium nitrate = Mg(NO3)2 Aluminum nitrate = Al(NO3)3</p> Signup and view all the answers

Dinitrogen pentoxide is represented by the formula N2O4.

<p>False (B)</p> Signup and view all the answers

Write the chemical formula for lithium bromide.

<p>LiBr</p> Signup and view all the answers

The mass number of an isotope is the sum of its protons and ______.

<p>neutrons</p> Signup and view all the answers

What is the mass number of carbon-14?

<p>14 (D)</p> Signup and view all the answers

What is the mass number of Carbon with 6 protons?

<p>12 (C)</p> Signup and view all the answers

A physical property can involve a change in composition.

<p>False (B)</p> Signup and view all the answers

How many neutrons are in Nitrogen-15?

<p>8</p> Signup and view all the answers

The acronym for a solution is _.

<p>aq</p> Signup and view all the answers

Match the following to their definitions:

<p>Element = Pure substance made of only one type of atom Mixture = Combination of two or more substances Compound = Substance formed when two or more elements are chemically bonded Solution = Homogeneous mixture of solute and solvent</p> Signup and view all the answers

Which element is most likely to form a negative ion?

<p>Chlorine (Cl) (D)</p> Signup and view all the answers

Strong acids do not ionize completely in water.

<p>False (B)</p> Signup and view all the answers

What is an example of a strong base?

<p>Sodium Hydroxide (NaOH)</p> Signup and view all the answers

The part of the periodic table containing metals that usually lose electrons is called the _ metals.

<p>alkali</p> Signup and view all the answers

Which of the following is a characteristic of a heterogeneous mixture?

<p>Can be separated by filtration (A)</p> Signup and view all the answers

Flashcards

Molar Mass

The mass of one mole of a substance. It is calculated by adding the atomic masses of all the atoms in the chemical formula.

Empirical Formula

The smallest whole-number ratio of atoms in a compound. It is a simplified version of the molecular formula.

Molecular Formula

The actual number of atoms of each element in a molecule.

Dimensional Analysis

A method used to convert between different units. It involves multiplying a given value by a conversion factor to obtain the desired unit.

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Density

The ratio of the mass of a compound to its volume.

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Percent Composition

The percentage by mass of each element in a compound.

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Avogadro's Number

The number of atoms, molecules, or any other specified particles in one mole of a substance.

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Limiting Reactant

The reactant that is completely consumed in a chemical reaction and limits the amount of product that can be formed.

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Theoretical Yield

The maximum amount of product that can be produced from a given amount of reactants, based on the limiting reactant.

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Actual Yield

The actual amount of product obtained in a chemical reaction, which may be less than the theoretical yield due to factors like incomplete reactions or side reactions.

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Percent Yield

The ratio of the actual yield to the theoretical yield, expressed as a percentage. It indicates the efficiency of a chemical reaction.

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Balanced Chemical Equation

A chemical equation that represents the chemical reaction involved, showing the reactants and products with their stoichiometric coefficients.

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Stoichiometric Ratio

The ratio of moles of reactants and products in a balanced chemical equation. It indicates the relative amounts of substances involved in the reaction.

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Stoichiometry

A method used to calculate the mass of a substance needed or produced in a chemical reaction, using the balanced chemical equation and the molar mass of the substances involved.

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Ionic Compound

A compound formed from the reaction of a metal and a nonmetal, where the metal loses electrons to become a cation and the nonmetal gains electrons to become an anion.

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Covalent Compound

A compound formed from the reaction of two nonmetals, where they share electrons to form covalent bonds.

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Binary Acid

A compound formed from the reaction of hydrogen with a nonmetallic anion.

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Oxyacid

An acid containing oxygen, hydrogen, and another nonmetal.

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Ionic Compound Hydrate

A compound composed of an ionic compound and water molecules, with the water molecules attached to the ionic compound.

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Isotope

A form of an element that has the same number of protons but a different number of neutrons.

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Mass Number

The sum of the protons and neutrons in an atom.

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Atomic Number

The number of protons in the nucleus of an atom.

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Number of Neutrons

The number of neutrons in the nucleus of an atom.

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Number of Electrons

The number of electrons in a neutral atom.

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Wave Energy and Frequency

The energy carried by a wave is directly proportional to its frequency. Higher frequency waves have higher energy.

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Frequency and Wavelength Relationship

A higher frequency wave will have a shorter wavelength.

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Electromagnetic Spectrum

The electromagnetic spectrum describes all the different types of light waves. It is organized by frequency, wavelength, and energy. Gamma rays have the highest energy and shortest wavelength, while radio waves have the lowest energy and longest wavelength.

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Bohr Model of the Atom

The Bohr model describes how electrons orbit the nucleus of an atom in specific energy levels. Electrons can jump between these energy levels by absorbing or releasing energy in the form of light.

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Atomic Orbitals

Electrons in atoms are organized into different subshells (s, p, d, f) and orbitals within those subshells. Orbitals have specific shapes and hold a maximum of two electrons.

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Chemical Property

A change in the composition of a substance, resulting in a new substance with different properties.

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Physical Property

A characteristic of a substance that can be observed or measured without changing its chemical composition.

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Element

A substance composed of only one type of atom, found on the periodic table (e.g., sodium (Na), oxygen (O)).

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Compound

A substance made of two or more elements chemically combined in a fixed ratio (e.g., water (H2O), table salt (NaCl)).

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Homogeneous Mixture (Solution)

A mixture where components are evenly distributed and indistinguishable (e.g., saltwater, air).

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Heterogeneous Mixture

A mixture where components are not evenly distributed and easily identifiable (e.g., sand in water, salad).

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Ion

Atoms that have gained or lost electrons, giving them a net positive or negative charge.

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Molecule

A group of atoms held together by chemical bonds.

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Study Notes

Determining Average Atomic Mass

  • Average atomic mass is calculated using the fractional abundance and isotopic mass of each isotope.
  • The equation is: average mass = ∑(fractional abundance × isotopic mass)
  • Convert percent abundances to decimal form.

Percent Composition

  • The percent composition of an element in a compound is calculated by dividing the mass of the element by the total mass of the compound, then multiplying by 100%.
  • The equation is: % = (part/whole) × 100%

Determining Empirical and Molecular Formulas

  • To determine a molecular formula, you need the empirical formula, the molar mass of the compound, and the ratio of molar mass to empirical mass.
  • The ratio of molar mass to empirical mass is used to multiply the empirical formula to get the molecular formula.
  • Molecular formula is the actual number of atoms of each element in a molecule of the compound.

Density

  • Density is mass divided by volume.
  • The unit for density is grams per cubic centimeter (g/cm³) or other equivalent units. Units for volume can include liters, milliliters, cubic meters, and so on.

Dimensional Analysis and Conversions

  • Dimensional analysis uses conversion factors to convert values from one unit to another.
  • A consistent set of units are used.
  • Examples include converting from nanometers to meters, or moles to grams.

Limiting Reactant

  • The limiting reactant is the reactant that is completely consumed in a chemical reaction and determines the amount of product that can be formed.
  • Calculate the mass of the products formed by each reactant first to determine the limiting reactant.

Balancing Chemical Equations

  • Chemical equations must be balanced to follow the law of conservation of mass.
  • This means the number of atoms of each element must be the same on both sides of the equation.

Naming Compounds

  • Transition metals, covalent compounds, binary acids, and oxyacids are all named differently.
  • Use Roman numerals for transition metals to specify the charge, use Greek prefixes for covalent compounds, use hydro- prefix for binary acids and specify the oxidation number by writing the name of the nonmetal with -ide.
  • Use the name of the nonmetal with an -ic ending for oxyacids.

Types of Reactions

  • Different types of reactions exist, including acid-base reactions, oxidation-reduction reactions, precipitation, combustion, gas forming, single-replacement, neutralization, decomposition, etc.

Isotopes

  • Isotopes are atoms of the same element that have the same number of protons and different numbers of neutrons.
  • They differ in mass number.
  • The mass number of an isotope is calculated by adding the number of protons and neutrons.

Physical and Chemical Properties

  • Physical properties are properties that can be measured without changing the chemical makeup of a substance.
    • Examples include: boiling point, melting point, density, color, odor, and malleability.
  • Chemical properties are properties that can only be observed by changing the chemical structure of a substance.
    • Examples include: reactivity, flammability, and the ability to corrode.

Atomic Structure and Properties

  • Atomic structure is explained by the Bohr Model.
  • Energy levels are considered in diagrams for absorption and emission of light.

Orbital Diagrams

  • Different types of orbitals with various shapes exist, each designated by x, y, and z coordinates.
  • Valence electrons and core electrons are parts of the atomic structure.
  • Valence electrons are electrons in the outermost energy level and play a significant role in chemical bonding.

Electron Configuration

  • Electron configuration refers to the arrangement of electrons in the different energy levels and orbitals within the atom.
  • Specific notations must be followed for electron configuration.

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