Chemistry Chapter 2 Quiz

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Questions and Answers

What describes the movement of particles in a solid?

  • Particles are far apart and move rapidly
  • Some vibrational movement but mostly stuck in place (correct)
  • Particles move freely and spread apart
  • Particles may slide past one another

Liquid has a definite shape and definite volume.

False (B)

What is the process called when a gas changes into a liquid?

Condensation

The phase change from solid to gas is called _____

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

Match each phase change with its corresponding description:

<p>Melting = Solid to Liquid Vaporization = Liquid to Gas Freezing = Liquid to Solid Deposition = Gas to Solid</p> Signup and view all the answers

What is the maximum number of questions on the first exam?

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

Students are allowed to eat or drink in the lab during experiments.

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

What should you do immediately after a spill occurs in the lab?

<p>Inform the teacher</p> Signup and view all the answers

Match the following lab safety rules with their description:

<p>Always read the lab = Prepare before starting experiments Keep work area clean = Prevent accidents with a tidy space Handle glassware with care = Avoid breakage and injuries Never eat or drink in lab = Maintain a safe environment</p> Signup and view all the answers

How many total valence electrons are present in the HCl compound?

<p>8 (B)</p> Signup and view all the answers

Dashes in a Lewis Structure represent single valence electrons.

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

What is the total number of valence electrons in an oxygen molecule (O2)?

<p>12</p> Signup and view all the answers

To fulfill the octet rule, an atom must have _____ valence electrons.

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

Match the following compounds with their total valence electrons:

<p>H2 = 2 H2O = 8 NH3 = 8 CCl4 = 32</p> Signup and view all the answers

Which of the following prefixes represents a factor of one thousand?

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

The unit 'grams' is commonly used in physics.

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

What is the term for the bottom curve of a liquid in a graduated cylinder that should be used for measuring volume?

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

A substance with a greater density than water will __________.

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

Match the separation technique with its description:

<p>Filtration = Separating based on particle size Evaporation = Separating based on boiling point Chromatography = Separating based on solubility Decantation = Separating based on density</p> Signup and view all the answers

Which of the following is NOT one of the four classifications of matter?

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

A mixture that has a uniform composition throughout is known as a heterogeneous mixture.

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

What is Archimedes' principle used for?

<p>Calculating volume, density, or mass of an object</p> Signup and view all the answers

A __________ is the part of a solution that gets dissolved.

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

Which of the following is an example of a diatomic molecule?

<p>N2 (D)</p> Signup and view all the answers

Which of the following is the correct suffix change for nonmetals in binary compounds?

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

In covalent bonding, the prefix 'mono-' can be used for the first element.

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

What step is used to indicate the charge of a transition metal when naming Type II binary compounds?

<p>Use a Roman Numeral</p> Signup and view all the answers

In a Lewis structure, each _______ represents 2 valence electrons being shared.

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

Which of the following prefixes represents four atoms in a covalent compound?

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

Match the following terms with their definitions:

<p>Lewis Dot Structure = Representation of valence electrons using dots Covalent Bonding = Sharing of electrons between atoms Transition Metal = Metal that can form multiple charges Polyatomic Ion = Ion consisting of two or more atoms</p> Signup and view all the answers

List one rule for counting significant figures.

<p>Non-zero digits are always significant.</p> Signup and view all the answers

In significant figures, zeros located between non-zero digits are ______.

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

Which of the following indicates a chemical change?

<p>A color change occurs. (B)</p> Signup and view all the answers

Electrons are found in the nucleus of an atom.

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

What is the charge of a cation?

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

The chemical family of elements in Group 2 is called the ________.

<p>Alkaline Earth Metals</p> Signup and view all the answers

Which period on the periodic table defines the energy level of valence electrons?

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

Increases in atomic radius occur from left to right in a period.

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

Name the two types of ions.

<p>Cations and Anions</p> Signup and view all the answers

Elements in Group 17 are known as ________.

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

Which of these elements has the largest ionization energy?

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

All elements in Group 18 do not form a charge because they have a full valence shell.

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

What shape does an S orbital have?

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

The ________ principle states that atomic radius increases from top to bottom in a group.

<p>atomic radius</p> Signup and view all the answers

Match the following groups with their corresponding family names:

<p>Group 1 = Alkali Metals Group 2 = Alkaline Earth Metals Group 15 = Nitrogen Group Group 16 = Chalcogens</p> Signup and view all the answers

Flashcards

Lab Safety Rules

A set of rules that must be followed during experiments to ensure safety and prevent accidents.

Pre-Lab Assignment

The process of carefully reading and understanding an experiment's instructions before starting.

Potential Risks

Recognizing and understanding potential hazards, such as flammable or toxic substances, present in a lab.

Keep Work Area Clean

Maintaining a clean and organized workspace to prevent accidents and ensure accurate results.

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Handle Glassware and Heating Sources With Caution

Handling fragile equipment with care and using heating sources cautiously to avoid injuries or damage.

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Melting

The process of a solid changing into a liquid.

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Vaporization

The process of a liquid changing into a gas.

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Condensation

The process of a gas changing into a liquid.

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Freezing

The process of a liquid changing into a solid.

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Sublimation

The process of a solid changing directly into a gas without going through a liquid state.

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Atom

The smallest unit of an element that still retains the chemical properties of that element. It is composed of a nucleus containing protons and neutrons, surrounded by a cloud of electrons.

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Element

A pure substance that cannot be broken down into simpler substances by chemical means. It is made up of only one type of atom.

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Compound

A substance formed when two or more different elements combine chemically in a fixed ratio. They have properties distinct from the elements they are composed of.

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Homogeneous Mixture

A mixture where the components are evenly distributed throughout. The individual components cannot be easily distinguished, and it appears uniform.

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Heterogeneous Mixture

A mixture where the components are not evenly distributed. The individual components can be easily distinguished, and it often appears as a suspension or a precipitate.

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Solute

A substance that dissolves in a solvent to form a solution. It typically changes state.

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Solvent

A substance that dissolves a solute to form a solution. It typically does not change state and is present in a larger amount than the solute.

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Mass

The amount of matter in an object.

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Volume

The amount of space an object occupies.

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Density

A measure of how much mass is contained in a given volume.

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Valence electrons in a molecule

The total number of valence electrons in a molecule can be calculated by adding up the number of valence electrons for each atom in the molecule.

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Lewis Structure

The Lewis Structure is a diagram that shows the bonding between atoms in a molecule and the lone pairs of electrons that may exist in the molecule.

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Dashes in Lewis Structure

A dash represents a bond between 2 atoms, which means 2 valence electrons shared.

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Dots in Lewis Structure

Dots represent single valence electrons that are not involved in bonding.

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Octet rule

The octet rule states that atoms tend to gain, lose, or share electrons to have 8 valence electrons in their outer shell. This makes them more stable.

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Chemical Change

Any change that results in the formation of a new substance with different chemical properties.

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Physical Change

A change in the physical appearance of a substance without altering its chemical composition.

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Protons

Positively charged particles found in an atom's nucleus, determining the element's identity.

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Neutrons

Neutral particles found in an atom's nucleus, contributing to its mass.

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Isotopes

Atoms of the same element with different numbers of neutrons, leading to variations in mass.

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Electrons

Negatively charged particles orbiting an atom's nucleus in electron clouds, sometimes involved in chemical reactions.

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Ions

Atoms that have gained or lost electrons, resulting in a net positive or negative charge.

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Cations

Positively charged ions with more protons than electrons.

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Anions

Negatively charged ions with more electrons than protons.

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Metals

Elements found on the left side of the Periodic Table, typically shiny, malleable, and good conductors of heat and electricity.

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Metalloids

Elements found along the stair-step line of the Periodic Table, possessing properties of both metals and nonmetals.

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Nonmetals

Elements found on the right side of the Periodic Table, generally poor conductors of heat and electricity, and often gases at room temperature.

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Period

The horizontal rows of the Periodic Table, representing the increasing energy levels of an atom's valence electrons.

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Group

The vertical columns of the Periodic Table, representing the number of valence electrons an atom has.

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Valence Electrons

Electrons found in the outermost shell of an atom, which participate in chemical reactions.

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Naming Type II Binary Compounds

In a type II binary compound, the metal element is written first and followed by a Roman numeral to indicate its charge. The nonmetal element's suffix is changed to -ide.

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Covalent Nomenclature

In covalent compounds, the less electronegative element is written first, followed by the more electronegative element. Prefixes are used to indicate the number of atoms of each element. The second element's suffix is changed to -ide, unless it is a polyatomic ion.

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Lewis Dot Structures

The number of dots around an element symbol represents the number of valence electrons. Each line in covalent compounds represents two shared valence electrons.

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Electron Pairing in Covalent Compounds

Each dot in a Lewis Dot structure represents one valence electron, while each line represents two shared electrons.

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Significant Figures

The number of significant figures indicates the precision of a measurement. For example, a measurement of 0.0150 cm has three significant figures, indicating precision up to the thousandth decimal place.

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Rules for Counting Significant Figures

Significant figures are used to express the precision of measured values. Non-zero digits are always significant. Leading zeros are not significant. Trailing zeros are significant only if they appear after a decimal point. Trailing zeros are not significant if they follow a decimal point.

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Laboratory Equipment

A beaker is used to hold liquids, while a graduated cylinder is used to measure liquid volumes with precision. A thermometer measures temperature. A ruler measures length. Electronic balances measure mass.

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Identifying Chemical Hazards

Chemical hazards can be classified as flammable, corrosive, toxic, or reactive.

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Study Notes

Pre-Comprehensive Study Guide Directions

  • Print name and element on the page.
  • Pre-Comprehensive Periodic Table is in the packet.
  • Scientific calculator and periodic table allowed during the exam. Ensure familiarity with calculator and table use.
  • Study guide divided into two sections: Key Topics to Review (pages 3-10) and Practice Problems (pages 11-25).
  • Key Topics is a review of major points from class notes; more in-depth review of notes recommended for confidence.
  • Practice Problems provide examples of potential pre-comp exam questions.

Helpful Reminders

  • Read entire study guide before beginning work.
  • Prioritize studying weakest topics (allocate ~20 minutes nightly).
  • Attend study sessions for questions.
  • Annotate the guide (highlighting important concepts, noting points for review in notes).
  • Utilize previous worksheets, tests, and Do Now assignments.

Lab Safety Rules and Key Topics to Review

  • Read lab assignments and perform pre-lab assignments before the experiment.
  • Be aware of potential risks (e.g., flammability, toxicity).
  • Maintain a clean and clear work area.
  • Carefully handle glassware and heating sources.
  • No horseplay to avoid accidents.
  • Do not eat or drink in the lab.
  • Inform teacher of spills or breakages immediately.
  • Never dispose of chemicals down the sink without specific instruction.
  • Chemical exposure prevention involves three pathways: absorption, ingestion, and inhalation. Methods to mitigate chemical exposure include: wearing protective eyewear, avoiding contact lenses in lab, wearing closed-toe shoes, tying back hair, wearing gloves, and wearing long sleeves/pants.
  • Be able to identify Globally Harmonized Safety (GHS) Symbols.

Key Topics to Review (cont'd)

  • National Fire Protection Agency (NFPA) Labels: Understand the meaning of the colors on NFPA labels (blue - health hazard, yellow - reactivity, red - flammability, white - special warning). Know the meaning of COR and W in NFPA labels. Learn what each number on the label means in terms of hazard levels.
  • Emergency Equipment: Be familiar with the functions and circumstances of using fire extinguishers, fire blankets, fire alarms, gas shutoffs, safety showers, fume hoods, and eyewash stations.
  • Lab Tools: Know the purpose and identification of various lab tools (mass balance, graduated cylinder, Erlenmeyer flask, beaker, test tube, volumetric flask, Bunsen burner, hot plate, watch glass, pipette, funnel, thermometer).
  • Unit Conversions: Be able to convert units involving prefixes (e.g., kilo-, deca-, milli-) to base units and vice versa. Also, conversion between different prefixed units.

SI Units and Chemistry Units

  • Know SI units (kilogram, meters, meters cubed, seconds, Kelvin).
  • Know common chemistry units (grams, milliliters, centimeters cubed, Kelvin, Celsius).

Accuracy vs. Precision

  • Accuracy: hits the mark even if not consistent
  • Precision: shows consistency but isn't necessarily accurate

Measuring Volume Precisely

  • Understand how to measure volumes using lab tools and the concept of the meniscus.

Density

  • Understand the relationship between mass, volume, and density.
  • Calculating density from two of the three variables correctly.
  • Identifying the substance with greater/lesser density will sink/float.

Archimedes Principle & Displacement

  • Calculate the volume, density, or mass of an object using Archimedes Principle (Vobject = Vfinal – Vinitial).

Classifying Matter

  • Classifying substances (element, compound, heterogeneous/homogeneous mixture).
  • Identifying different parts of mixtures: solute, solvent
  • Understanding compounds and mixtures
  • Separation techniques (filtration, evaporation, chromatography, decantation).

States of Matter

  • Compare and contrast solids, liquids, and gases in terms of energy, movement, shape, and volume.
  • Identify the states of matter using diagrams.
  • Understand phase changes.

Physical vs. Chemical Changes

  • Identify physical (extensive/intensive properties, phase change) and chemical changes.

Atomic Structure

  • Understand the properties of subatomic particles (protons, neutrons, electrons, isotopes).
  • Understand how to calculate mass, valence electrons and charge of atoms.
  • Classifying metals, nonmetals, metalloids in the periodic table.
  • Understand periodic trends related to rows (periods) and columns (groups) of elements.
  • Understand nuclear notation for representing elements, isotopes, and ions.

Families of the Periodic Table

  • Identify elements in Alkali Metals, Alkaline Earth Metals, Transition Metals, Halogens, and Noble Gases families.
  • Identify Metalloids (families including B, Si, Ge, As, Sb, Te, and Po).
  • Predict the properties of elements, based on their location in the table.

Electronic Configuration of Atoms

  • Identify the number of valence electrons in an atom.
  • Define the most likely charge that an element's ion will assume.
  • Determine whether the ion will be a cation or anion.
  • Write standard and shorthand notation electron configuration of elements (e.g. standard notation CI: 1s22s22p63s²3p5 and shorthand notation CI: [Ne]3s23p5).

Ionic Bonding

  • Naming and writing the chemical formulas of ionic compounds.

Covalent Bonding

  • Naming and writing the chemical formulas of covalent compounds.

Lewis Structures

  • Draw Lewis dot structures for elements/compounds using correct configurations.

Unit 1: Laboratory Safety, Measurement, and Significant Figures

  • Identifying hazards / Lab safety.
  • Precision in measuring using lab equipment.
  • Calculating using significant figures.

Unit 2 & 3: Types, Properties, and States of Matter

  • Classifying matter (solids, liquids, gases).
  • Distinguishing properties of states of matter.
  • Understanding different types of matter (pure substances, mixtures, elements, compounds).

Unit 4: The Periodic Table

  • Identifying and filling in characteristics of different elements.

Unit 5: Chemical Bonding

  • Identifying types of bonds (ionic, covalent), and chemical formulas.

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