Physical Science Unit Conversions and Lab Safety
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Questions and Answers

What is weight a measure of?

  • The density of a substance
  • The mass of an object
  • The volume of a substance
  • The amount of gravity exerted on an object (correct)
  • A chemical change can be easily reversed.

    False

    List three examples of physical changes.

    Slicing bread, ice cream melting, plate breaking

    The four phases of matter are solid, liquid, gas, and ______.

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

    Which of the following is NOT an intensive property?

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

    Match the following phase changes with their definitions:

    <p>Sublimation = Solid to gas Melting = Solid to liquid Condensation = Gas to liquid Freezing = Liquid to solid</p> Signup and view all the answers

    What are three examples of chemical changes?

    <p>Baking a cake, egg frying, fireworks</p> Signup and view all the answers

    Intensive properties change when the amount of substance changes.

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

    What is the conversion of kilo to grams?

    <p>1 kilo = 1000 grams</p> Signup and view all the answers

    What is the formula for density?

    <p>Density = Mass / Volume</p> Signup and view all the answers

    Goggles should only be worn during experiments involving heat.

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

    What are the two branches of physical science?

    <p>Physics and chemistry</p> Signup and view all the answers

    To find the density of a regular solid, you divide the volume by the mass.

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

    Anything that has mass and takes up ________ is defined as matter.

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

    How do you find the density of an irregular solid?

    <p>You measure the mass and determine the volume by water displacement in a graduated cylinder, then divide the mass by the volume.</p> Signup and view all the answers

    Match the following separation techniques with their definitions:

    <p>Distillation = Separating based on boiling points Chromatography = Separating based on color or solubility Filtration = Separating solids from liquids Evaporation = Removes a liquid from a solution</p> Signup and view all the answers

    Boyle's Law is represented by the formula ___ = P2V2.

    <p>P1V1</p> Signup and view all the answers

    Which of the following are not considered matter?

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

    Match the laws with their relationships:

    <p>Boyle's Law = As pressure increases, volume decreases Charles's Law = As volume increases, temperature increases Density = Mass per unit volume Water Displacement = Finding volume of irregular shapes</p> Signup and view all the answers

    Elements and compounds are the two types of pure substances.

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

    What happens to the volume of a gas when its pressure increases, according to Boyle's Law?

    <p>It decreases</p> Signup and view all the answers

    The first action to take if there is an accident in the lab is to ________ the instructor immediately.

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

    Charles's Law states that volume and temperature are directly related for a gas.

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

    What is the difference between mass and weight?

    <p>Mass is the amount of matter in an object, while weight is the force exerted by gravity on that matter.</p> Signup and view all the answers

    What describes an ionic bond?

    <p>Involves the transfer of electrons</p> Signup and view all the answers

    The mass number of an isotope is represented by the bottom number in its formula.

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

    The prefixes for a covalent compound include 1-, 2-, and 3-____.

    <p>mono, di, tri</p> Signup and view all the answers

    Match the type of bond with its description:

    <p>Ionic bond = Transfer of electrons between a metal and nonmetal Covalent bond = Sharing of electron pairs between nonmetals Metallic bond = Pooling of electrons among many atoms</p> Signup and view all the answers

    What represents isotopes?

    <p>Atoms of the same element with different mass numbers</p> Signup and view all the answers

    Periodic law states that elements listed in order of their atomic numbers fall into groups.

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

    List three indicators of a chemical reaction.

    <p>Color change, temperature change, gas/bubbles</p> Signup and view all the answers

    Which of the following processes describes the transition from gas to liquid?

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

    Bohr's atomic model suggests that electrons move in undefined paths around the nucleus.

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

    What did Rutherford discover about the structure of the atom?

    <p>Atoms are made mostly of empty space with a dense positively charged nucleus.</p> Signup and view all the answers

    The smallest part of a chemical element that can exist is called an _____

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

    Match the atomic models with their descriptions:

    <p>Dalton's Model = Atoms are uncuttable and identical for an element Thomson's Model = Positively charged substance with negatively charged particles Rutherford's Model = Atoms consist of mostly empty space Bohr's Model = Electrons in definite orbits around the nucleus</p> Signup and view all the answers

    Which particle carries a negative charge?

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

    In Dalton's atomic theory, atoms of the same element are always different.

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

    The process of gas changing directly to solid is called _____

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

    What is the general equation for a synthesis reaction?

    <p>A + B = AB</p> Signup and view all the answers

    In a decomposition reaction, one product will yield two or more products.

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

    What is the definition of an acid/base reaction?

    <p>An acid and a base react to form a salt; it involves neutralization.</p> Signup and view all the answers

    In a combustion reaction, a reactant combines with _____ to produce water and carbon dioxide.

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

    Which of the following is a correct description of a double replacement reaction?

    <p>2 reactants yield 2 products; reactants and products are flipped</p> Signup and view all the answers

    What does pH stand for?

    <p>Potential of Hydrogen</p> Signup and view all the answers

    Match the following types of reactions with their definitions:

    <p>Synthesis = 2 reactants yielding 1 product Decomposition = 1 product yields 2 or more products Combustion = Reactant + oxygen = water and carbon dioxide Single replacement = 2 reactants = 2 products; 1 reactant and product are flipped</p> Signup and view all the answers

    In chemistry, OH- is associated with a _____ and H+ is associated with an _____ in a reaction.

    <p>base, acid</p> Signup and view all the answers

    Study Notes

    Unit Conversions

    • 1000 milli = 1 gram
    • 100 centi = 1 gram
    • 1 kilo = 1000 grams

    Lab Safety

    • Wear goggles when working with chemicals, heat, and glassware
    • Immediately notify instructor if there's a chemical in eyes or on skin
    • Flush affected area with water from eye wash station or safety shower for 20 minutes

    Accidents in the Lab

    • Follow specific steps in case of lab accidents

    Physical Science

    • Study of non-living things
    • Branches are Physics and Chemistry

    Matter

    • Anything that has mass and takes up space
    • Examples of things that are not matter: time, energy, and light

    Separation Techniques

    • Distillation
    • Chromatography
    • Filtration

    Pure Substances

    • Elements
    • Compounds

    Mixtures

    • Heterogeneous (not mixed)
    • Homogeneous (well mixed)

    Density

    • Mass per unit volume (m/v)
    • Regular solid: Measure mass and dimensions, calculate volume, then divide mass by volume
    • Irregular solid: Measure mass, use water displacement to find volume, then divide mass by volume
    • Liquid: Measure mass of known volume of liquid, then divide mass by volume

    Boyle's Law

    • P1V1 = P2V2
    • Pressure and volume are inversely related

    Charles's Law

    • V1/T1 = V2/T2
    • Volume and temperature are directly related

    Mass vs Weight

    • Mass: amount of matter in an object
    • Weight: measure of gravitational force on an object

    Physical Changes

    • Influence form of substance but not identity
    • Easily reversed
    • Example: change of phase (intensive property)

    Intensive Properties

    • Density, melting point, color

    Chemical Changes

    • Cause by chemical reaction
    • Forms new substance with different properties
    • Not easily reversed
    • Examples: Baking a cake, egg frying, fireworks

    Phases of Matter

    • Solid
    • Liquid
    • Gas
    • Plasma

    Phase Changes

    • Solid to gas = sublimation
    • Solid to liquid = melting
    • Liquid to solid = freezing
    • Gas to solid = deposition
    • Gas to liquid = condensation
    • Liquid to gas = vaporization
    • Gas to plasma = ionization
    • Plasma to gas = recombination

    Atoms

    • Smallest part of a chemical element

    Dalton's Atomic Theory

    • Atoms are uncuttable
    • Atoms of the same element are alike

    Thomson's Atomic Model

    • Positively charged substance with negatively charged particles scattered (chocolate chip cookie)

    Rutherford's Discovery

    • Atoms are mostly empty space with a dense, positively charged nucleus

    Bohr's Atomic Model

    • Electrons move in definite orbits (solar system)
    • Protons, Neutrons in nucleus, electrons outside

    Subatomic Particles

    • Proton (+), Neutron (0), Electron (-)

    Atomic Number vs Mass Number

    • Atomic number = Number of protons
    • Mass number = Number of protons + neutrons

    Groups on the Periodic Table

    • Alkali metals (Group 1)
    • Alkaline earth metals (Group 2)
    • Halogens (Group 7A, 17)
    • Noble gases (Group 8A, 18)
    • Transition metals (Groups 3-12)
    • Metalloids (along the staircase)

    Ionic Bonds

    • Metal and nonmetal
    • Use charges and add "ide" to nonmetal name

    Covalent Bonds

    • Two nonmetals
    • Use prefixes based on number of atoms

    Isotopes

    • Top number = Mass number
    • Bottom number = Atomic number

    Periodic Law

    • When elements are listed in order of their atomic numbers, similarities in their properties occur periodically

    Valence Electrons

    • Electrons in the outermost shell

    Charges of Groups

    • Calculated based on the number of electrons gain or loss in order to be stable

    Chemical Formula Prefixes

    • 1-mono, 2-di, 3-tri, etc.

    Chemical Reactions (General)

    • Synthesis: 2 reactants combine to form 1 product (A + B → AB)
    • Decomposition: 1 reactant breaks down into 2 or more products (AB → A + B)
    • Single Replacement: One element replaces another in a compound (A + BC → AC + B)
    • Double Replacement: Two elements in different compounds exchange places (AB + CD → AD + CB)
    • Combustion: Substance reacts with oxygen to produce heat and light (usually creating water vapor and carbon dioxide)

    Acids and Bases

    • Acid: pH < 7
    • Base: pH > 7
    • Neutral: pH = 7

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    Semester Exam Study Guide PDF

    Description

    Test your knowledge on unit conversions, lab safety protocols, and fundamental concepts in physical science. This quiz covers essential topics such as matter, pure substances, mixtures, and separation techniques. Challenge yourself to ensure a safe and successful laboratory experience!

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