Campbell Bio Ch 2+3
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Questions and Answers

Match the following elements with their primary roles in living organisms:

Oxygen = Makes up 96% of living matter Calcium = Essential for bone structure Nitrogen = Key component of amino acids Potassium = Regulates fluid balance

Match the following types of substances with their definitions:

Element = A substance that can't be broken down Compound = A substance made of two or more different atoms Trace Element = An element present in small quantities Toxic Element = An element that can be harmful to living organisms

Match the following biological needs with the corresponding life forms:

Humans = Need 25 elements to sustain life Plants = Need 17 elements to sustain life Animals = Evolved tolerance to toxic elements All living organisms = Require 20-25% of elements from the periodic table

Match the following groups of elements with their percentage contribution to living matter:

<p>Oxygen, Carbon, Hydrogen, Nitrogen = 96% of living matter Calcium, Phosphorus, Potassium, Sulfur = Remaining 4% of living matter Hydrogen = Part of most organic compounds Carbon = The backbone of organic molecules</p> Signup and view all the answers

Match the following statements with their correct concepts:

<p>Living organisms = Contain a mix of essential elements Trace elements = Vital in small amounts for certain functions Compounds = Formed by bonding of different elements Periodic table = Contains 92 elements important for life</p> Signup and view all the answers

Match the following elements with their group in living matter:

<p>Oxygen = 96% of living matter Nitrogen = 96% of living matter Calcium = 4% of living matter Sulfur = 4% of living matter</p> Signup and view all the answers

Match the following subatomic particles with their charges:

<p>Protons = Positive charge Electrons = Circulate around the nucleus Neutrons = No charge</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Atomic Number = Number of protons in an atom Mass Number = Total number of protons and neutrons Atomic Mass = Mass of an atom, often a decimal Isotopes = Atoms with differing numbers of neutrons</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Proton = Positively charged subatomic particle Neutron = Subatomic particle with no charge Electron = Negatively charged subatomic particle Atomic Number = Number of protons in an atom</p> Signup and view all the answers

Match the following concepts with their descriptions:

<p>Half-life = Time it takes for half of a radioactive isotope to decay Isotopes = Atoms with the same number of protons but different neutrons Radioactive Isotope = Unstable isotope that decays and releases energy Atomic Mass = Average mass of an atom, including isotopes</p> Signup and view all the answers

Match the following types of isotopes with their characteristics:

<p>Stable Isotope = Does not decay Radioactive Isotope = Nucleus decays, emits energy Mother Isotope = Original radioactive element Daughter Isotope = New element from decay process</p> Signup and view all the answers

Match the following scientific measurements with their descriptions:

<p>Half-life = Time for half of a substance to decay Dalton = Unit of measurement for atomic particles Atomic Mass = Average mass accounting for isotopes Radioactive Tracers = Used to track biological processes</p> Signup and view all the answers

Match the following shells with their electron capacity:

<p>First shell = Can hold 2 electrons Second shell = Can hold 8 electrons Valence shell = Outermost electron shell Orbital = Area where an electron is found 90% of the time</p> Signup and view all the answers

Match the following particles with their location:

<p>Protons = Inside the atomic nucleus Neutrons = Inside the atomic nucleus Electrons = Circulate around the nucleus Nucleus = Contains protons and neutrons</p> Signup and view all the answers

Match the following types of isotopes with their characteristics:

<p>Mother Isotope = Original radioactive isotope before decay Daughter Isotope = Element formed after decay of mother isotope Stable Isotope = Does not undergo radioactive decay Unstable Isotope = Undergoes decay and changes into a different element</p> Signup and view all the answers

Match the following forms of electron shells with their orbital shapes:

<p>First shell = 1 spherical orbital Second shell = 1 spherical and 3 dumbbell orbitals Third shell = Multiple orbitals including s and p Valence shell = Contains the outermost electrons</p> Signup and view all the answers

Match the following types of elements with their definition:

<p>Trace Elements = Present in small quantities Toxic Elements = Natural elements that may be harmful Primary Elements = Make up the majority of living matter Secondary Elements = Contribute to the rest of living matter</p> Signup and view all the answers

Match the following concepts with their descriptions:

<p>Decay Process = Involves neutron converting to a proton Energy Release = Occurs during radioactive decay Stable vs Unstable Isotopes = Impact on element properties Tracking Metabolism = Use of radioactive tracers</p> Signup and view all the answers

Match the following statements with their implications:

<p>Electrons further from nucleus = Higher potential energy Full valence shell = Element is mostly unresponsive to reactions Unpaired electrons = Increase reactivity of an atom Chemical behavior = Dependent on electron distribution</p> Signup and view all the answers

Match the following terms with their occurrence in atoms:

<p>Isotopes = Same element, different neutrons Electrons = Form area of negative charge Atomic composition = Includes protons and neutrons</p> Signup and view all the answers

Match these processes with their outcomes:

<p>Neutron decay = Changes neutron to proton and alters element Energy release from electron = Usually emitted as light or radiation Atom's nucleus stability = Depends on number of protons and neutrons Chemical reactions = Involve electron interactions rather than nucleus</p> Signup and view all the answers

Match the following types of energy with their characteristics:

<p>Potential Energy = Stored energy due to position Kinetic Energy = Energy of motion Thermal Energy = Energy related to temperature Radiant Energy = Energy carried by light</p> Signup and view all the answers

Match the following applications of radioactive isotopes with their use:

<p>PET scan = Tracks metabolism through radioactive tracers Radiometric dating = Determines age of rocks and fossils Radioactive tracers = Used to track biochemical processes Medical imaging = Uses radioactive materials to visualize internal structures</p> Signup and view all the answers

Match the following types of chemical bonds with their characteristics:

<p>Nonpolar Covalent Bond = Atoms have the same level of electronegativity Polar Covalent Bond = Atoms have different electronegativities Ionic Bond = Results from the transfer of electrons Hydrogen Bond = Attraction between hydrogen and an electronegative atom</p> Signup and view all the answers

Match the following terms related to atomic structure:

<p>Electron Shell = An energy level where electrons reside Valence Shell = The outermost electron shell of an atom Orbital = A region where an electron is likely found Half-life = Time taken for half of a radioactive sample to decay</p> Signup and view all the answers

Match the following pairs of chemical structures:

<p>Lewis Dot Structure = Representation of electrons as dots around elements Structural Formula = Representation of bonds using lines between atoms Double Bond = Bond involving the sharing of two pairs of electrons Ion = An atom with a net electric charge due to loss or gain of electrons</p> Signup and view all the answers

Match the following elemental properties:

<p>Cation = Positively charged ion Anion = Negatively charged ion Salt = Compound formed from ionic bonds Crystals = Natural form of ionic compounds</p> Signup and view all the answers

Match the following statements about chemical reactions:

<p>Weak Chemical Reactions = Easily reversible interactions between atoms Energy = Capacity to cause change or do work Chemical Bonds = Interactions that hold atoms together Reactivity = Dependent on unpaired electrons in orbitals</p> Signup and view all the answers

Match the following terms related to electron configuration:

<p>Valence Electrons = Electrons in the outermost shell Electrons = Negatively charged particles around the nucleus Orbital Types = Regions where electrons are likely to be found Spherical Orbital = Found in the first electron shell</p> Signup and view all the answers

Match the following chemical concepts with their explanations:

<p>Hybridization = Mixing of atomic orbitals to form new hybrid orbitals Stability in Salts = More stable dry and can dissolve in water Hydrogen Bonding = Involves hydrogen with an electronegative atom Electrons in Shells = Can only exist on defined energy levels</p> Signup and view all the answers

Match the following characteristics of atoms:

<p>Incomplete Electron Shell = Causes atoms to interact and form bonds Full Valence Shell = Atoms are mostly unresponsive in reactions Atomic Orbitals = Regions where electrons drift around the nucleus Energy Levels = Determine the structure of electron shells</p> Signup and view all the answers

Match the following bonding concepts:

<p>Ionic Compounds = Formed through ionic bonds and not covalent bonds Crystal Form = Natural state of ionic compounds like salts Dry Ionic Bonds = Stronger when not shielded by solvents Dissolved in Water = Ionic bonds become weaker</p> Signup and view all the answers

Match the following bonding types with examples:

<p>Covalent Bond Example = H2 molecule formed by sharing electrons Ionic Bond Example = NaCl formed through electron transfer Nonpolar Covalent Example = O2 bonded by equal electronegativity Polar Covalent Example = Water molecule with unequal electron sharing</p> Signup and view all the answers

Match the following chemical attributes:

<p>Atomic Number = Number of protons in the nucleus Mass Number = Total number of protons and neutrons Isotope = Variations of an element with different neutrons Radioactive Decay = Process of an unstable nucleus losing energy</p> Signup and view all the answers

Match the following terms with their respective charges:

<p>𝛅+ = Indicates a partial positive charge 𝛅- = Indicates a partial negative charge Cation charge = Positive charge due to electron loss Anion charge = Negative charge due to electron gain</p> Signup and view all the answers

Match the following chemical bond types with their descriptions:

<p>Covalent Bond = Sharing of electron pairs between atoms Ionic Bond = Attraction between oppositely charged ions Polar Covalent Bond = Unequal sharing of electrons between atoms Nonpolar Covalent Bond = Equal sharing of electrons between identical atoms</p> Signup and view all the answers

Match the following types of bonds with their features:

<p>Hydrogen Bond = Attraction between a hydrogen atom and an electronegative atom Van der Waals Interactions = Weak forces between nonpolar molecules causing adhesion Double Bond = Sharing of two pairs of electrons between two atoms Ionic Compound = Formed from ionic bonds and usually crystallized</p> Signup and view all the answers

Match the following molecular shapes with their bonding characteristics:

<p>Tetrahedral = Four hybrid orbitals arranged in a pyramid shape Linear = Atoms arranged in a straight line Trigonal Planar = Three atoms bonded to one central atom in a flat plane Bent = Molecular shape with two atoms and one lone pair</p> Signup and view all the answers

Match the following types of chemical interactions with their examples:

<p>Ionic Bond = NaCl Hydrogen Bond = Water molecules Covalent Bond = H2 Van der Waals Interaction = Gecko's ability to climb surfaces</p> Signup and view all the answers

Match the following statements about compounds with their appropriate terms:

<p>Salts = Compounds formed from ionic bonds Molecules = Formed by covalent bonds Ionic Compounds = Do not consist of covalent bonds Weak Chemical Reactions = Easily reversible interactions</p> Signup and view all the answers

Match the following terms with their characteristics:

<p>Anion = Negatively charged ion Molecular Shape = Influences how a molecule interacts with others Lewis Dot Structure = Represents electrons as dots around symbols Structural Formula = Uses lines to represent bonds between atoms</p> Signup and view all the answers

Match the following types of covalent bonds with their examples:

<p>Double Bond = O2 (Oxygen gas) Single Bond = Hydrogen molecule (H2) Triple Bond = Nitrogen gas (N2) Polar Covalent Bond = Water (H2O)</p> Signup and view all the answers

Match the following concepts with their applications:

<p>Electronegativity = Determines bond polarity Covalent Bonds = Join nonmetals in molecules Ionic Bonds = Form between metals and nonmetals Hybrid Orbitals = Shape and arrangement of molecules</p> Signup and view all the answers

Match the following chemical properties with their corresponding bonds:

<p>Ionic Bond = Strength increases when dry Covalent Bond = Shares electrons to fill shells Hydrogen Bond = Forms between hydrogen and electronegative atoms Van der Waals Forces = Temporary dipoles in nonpolar molecules</p> Signup and view all the answers

Match the following drug interactions with their structural similarities:

<p>Morphine = Resembles natural endorphins in the brain Heroin = Analog to natural pain-relieving substances Opiate Drugs = Interact with neurotransmitter systems Endorphins = Produced naturally by the brain</p> Signup and view all the answers

Match the states of water with their properties:

<p>Liquid Water = Constantly forming and breaking bonds Ice = Less dense due to structured hydrogen bonds Water Vapor = Molecules move freely with high energy Supercooled Water = Liquid below freezing point without freezing</p> Signup and view all the answers

Match the following energy concepts with their definitions:

<p>Kinetic Energy = Energy from the movement of molecules Temperature = Average kinetic energy of a body of matter Heat = Transfer of thermal energy between bodies Calorie = Energy to raise temperature of water by one degree Celsius</p> Signup and view all the answers

Match the following types of bonds with their characteristics:

<p>Polar Covalent Bonds = Unequal sharing of electrons Hydrogen Bonds = Weak attraction between polar molecules Ionic Bonds = Transfer of electrons from one atom to another Covalent Bonds = Sharing of electron pairs between atoms</p> Signup and view all the answers

Match the following terms with their examples:

<p>Cohesion = Water beads on a surface Adhesion = Water climbing up plant roots Surface Tension = Insects walking on water Chemical Equilibrium = Ammonia formation and decomposition</p> Signup and view all the answers

Match the following temperatures with their comparative statements:

<p>Swimming Pool = More thermal energy than a hot mug of coffee Boiling Water = Higher temperature than ice Ice Water = Higher kinetic energy than frozen ice Room Temperature = Lower energy than boiled water</p> Signup and view all the answers

Match the following properties of water with their implications:

<p>High Specific Heat = Regulates temperature smoothly High Latent Heat = Requires more energy to change states Density Anomaly = Ice floats on water surfaces Polarity = Solvent properties in biological systems</p> Signup and view all the answers

Match the following chemical reaction elements with their outcomes:

<p>Reactants = Substances before a reaction Products = Substances formed after a reaction Higher Concentration = Increases chance of collisions Reversible Reaction = Can shift between reactants and products</p> Signup and view all the answers

Match the following terms related to water with their correct definitions:

<p>Specific Heat = Heat needed to change temperature by one degree Celsius Heat of Vaporization = Heat needed to convert one gram of liquid to gas Transiency = Creation and destruction of hydrogen bonds Aqueous Solution = Solution where a solute is dissolved in water</p> Signup and view all the answers

Match the following components of solutions with their roles:

<p>Solvent = Substance that dissolves another substance Solute = Substance that is dissolved Sodium ions = Positively charged ions attracted to water's negative regions Chlorine ions = Negatively charged ions attracted to water's positive regions</p> Signup and view all the answers

Match the following processes involving water with their descriptions:

<p>Vaporization = Transition from liquid to gas Condensation = Transition from gas to liquid Evaporation = Cooling process as warmer molecules escape Freezing = Transition of liquid water to solid ice</p> Signup and view all the answers

Match the following concepts with their related characteristics:

<p>Hydrogen bonds = Created and destroyed easily in water Kinetic energy = Increases with temperature rise Heat absorption in summer = Water cools surrounding air Heat release in winter = Water heats surrounding air</p> Signup and view all the answers

Match the following scientific terms with their corresponding values:

<p>1 Joule = 0.239 calories 1 calorie = 4.184 Joules 580 calories = Heat needed to evaporate 1 gram of water at 25°C Higher specific heat = Water compared to other substances</p> Signup and view all the answers

Match the following aspects of water's behavior with their effects:

<p>Resistance to temperature change = Allows for stable climates High heat capacity = Absorbs heat without drastic temperature rise Insulation by ice = Protects aquatic life in winter Evaporation cooling = Cools bodies of plants and animals</p> Signup and view all the answers

Match the following terms related to water molecules with their definitions:

<p>Hydrogen bonds = Weak attractions between water molecules Transiency = Constant formation and breaking of hydrogen bonds Kinetic energy during heating = Increases collisions between molecules Intermolecular attractions = Hold water molecules closely together</p> Signup and view all the answers

Match the following thermal properties of water with their consequences:

<p>High specific heat = Buffers temperature changes in environments High heat of vaporization = Prevents overheating in organisms Cooling effect of evaporation = Reduces temperature in transpiration Temperature regulation in large bodies = Maintains stable ecosystems</p> Signup and view all the answers

Match the following scientific concepts with their outcomes:

<p>Heat released during condensation = Lower kinetic energy state Formation of vapor = Increased kinetic energy of molecules Ice floating = Insulates water below Water's hydrogen bonds = Increased heat absorption capacity</p> Signup and view all the answers

Match the following types of energy with their descriptions:

<p>Kinetic Energy = Energy from motion of molecules Thermal Energy = Total kinetic energy of a body of matter Heat = Transfer of thermal energy between bodies Temperature = Average kinetic energy of a substance</p> Signup and view all the answers

Match the following substances with their molecular mass:

<p>Hydrogen = 1 g/mol Carbon = 12 g/mol Sucrose = 342 g/mol Substance B = 10 g/mol</p> Signup and view all the answers

Match the following terms with examples:

<p>Hydrophilic = Cellulose in cotton towels Hydrophobic = Cooking oil Molar Solution = One mole of substance dissolved in water Calorie = Energy to raise temperature of 1 gram of water by 1°C</p> Signup and view all the answers

Match the following types of solutions with their descriptions:

<p>One Molar Solution = One mole of solute in one liter Dilute Solution = Low concentration of solute Concentrated Solution = High concentration of solute Isotonic Solution = Equal concentration inside and outside a cell</p> Signup and view all the answers

Match the molecular properties with their characteristics:

<p>Molecular Mass = Sum of all atomic masses in a molecule Avogadro's Number = 6.02 x 10^23 units per mole Caloric Value = Energy needed to raise temperature of water Molecule Size = Influences solubility in water</p> Signup and view all the answers

Match the following components of water's behavior with their results:

<p>High Specific Heat = Temperature stabilizes in environments High Surface Tension = Insects walking on water Water as a Solvent = Dissolution of ionic compounds Heat of Vaporization = Effectiveness of sweating for cooling</p> Signup and view all the answers

Match the following types of thermodynamic quantities with their definitions:

<p>Calorie = Energy to raise 1 g of water by 1°C Kilocalorie = Energy to raise 1 kg of water by 1°C Thermal Energy = Energy due to temperature and volume Heat Transfer = Movement of thermal energy between substances</p> Signup and view all the answers

Match the following terms with their descriptions regarding water properties:

<p>Specific Heat = The heat required to raise the temperature of a substance by 1°C Heat of Vaporization = The heat needed to convert 1 gram of liquid to gas Hydrogen Bonds = Weak attractions between water molecules Evaporative Cooling = Cooling that occurs when the warmest molecules evaporate</p> Signup and view all the answers

Match each concept related to temperature regulation with its explanation:

<p>High Specific Heat = Regulates land temperatures for life Heat Absorption by Water = Helps cool the air during summer Heat Release in Winter = Warms the air from the water body Insulating Ice = Prevents water below from freezing completely</p> Signup and view all the answers

Match the following processes with their characteristics:

<p>Condensation = Releases heat as water changes from gas to liquid Vaporization = Requires heat to convert liquid to gas Transiency = Creation and breaking of hydrogen bonds Evaporation = Loss of warmest molecules leading to cooling</p> Signup and view all the answers

Match types of heat transfer with their examples:

<p>Conduction = Direct contact transferring heat Convection = Heat transfer through liquid or gas movement Radiation = Heat transfer through electromagnetic waves Evaporation = Cooling via changing from liquid to gas</p> Signup and view all the answers

Match the following effects of water's properties with their descriptions:

<p>Regulation of Body Temperature = Through sweating and evaporative cooling High Heat of Vaporization = Prevents rapid evaporation from bodies of water Hydrogen Bonding = Allows water to remain liquid over a range of temperatures Density of Ice = Ice floats and insulates water below</p> Signup and view all the answers

Match the terms related to water's role in the environment with their implications:

<p>Evaporative Cooling = Helps plants and animals regulate temperatures Aquatic Thermoregulation = Stabilizes temperatures in aquatic environments Hydrogen Bonding = Allows for unique properties of water High Specific Heat = Maintains stable climates</p> Signup and view all the answers

Match the following scenarios to their respective water properties:

<p>Ice forming on top of water = Less dense than liquid water Water boiling = Requires high heat to change from liquid to gas Plant sweating = Utilizes evaporative cooling Ocean absorbing sunlight = Regulates coastal temperatures</p> Signup and view all the answers

Match the following types of heat exchange with examples in nature:

<p>Solar Heat Absorption = Water absorbs heat during the day Heat Release at Night = Water releases heat to the cooler air Evaporative Cooling in Plants = Leaves cool when water evaporates Steam Burns = Heat released during water vapor formation</p> Signup and view all the answers

Match the terms associated with the behavior of water molecules with their functions:

<p>Low Temperature = Increased likelihood of hydrogen bond formation High Kinetic Energy = Increases likelihood of vaporization Molecular attraction = Keeps water molecules close together Bond breaking = Occurs when heat is added, increasing kinetic energy</p> Signup and view all the answers

Match the following acids/bases with their characteristics:

<p>Strong Acid = An acid that completely dissociates in solution Weak Acid = An acid that reversibly releases/accepts hydrogen ions Strong Base = A base that significantly decreases hydrogen ion concentration Weak Base = A base that partially accepts hydrogen ions in solution</p> Signup and view all the answers

Match the following substances with their effects on pH:

<p>Acid = Increases hydrogen ion concentration in water Base = Decreases hydrogen ion concentration in water Carbonic Acid = Acts as a buffer in blood plasma to maintain pH Ammonia = React with hydrogen ions to reduce their concentration</p> Signup and view all the answers

Match the following molecules with their molecular mass in daltons:

<p>Hydrogen = 1 dalton Carbon = 12 daltons Sucrose = 342 daltons Water = 18 daltons</p> Signup and view all the answers

Match the following statements with their corresponding chemical concepts:

<p>Equilibrium = A state when hydrogen atoms are dislocated as quickly as reformed pH = A measure of hydrogen ion concentration in a solution Molar Solution = One mol of solute dissolved in enough water to make one liter Hydration Shell = Water molecules surround dissolved ions or molecules</p> Signup and view all the answers

Match the following ions with the processes they relate to:

<p>H+ = Contributes to acidity in a solution OH- = Contributes to basicity in a solution H2CO3 = The acid in the carbonic acid-buffer system HCO3- = The bicarbonate that can act to buffer pH changes</p> Signup and view all the answers

Match the following examples with their classifications:

<p>Cooking Oil = Hydrophobic substance Sugar = Hydrophilic substance Cellulose = Hydrophilic but not soluble in water Acetic Acid = Weak acid that can dissociate partially</p> Signup and view all the answers

Match the following chemical reactions with their outcomes:

<p>HCl + H2O = Forms H+ and Cl- ions NH3 + H+ = Forms NH4+ NaOH → Na+ + OH- = Dissociates to produce hydroxide ions H2CO3 ⇄ HCO3- + H+ = Responds to changes in blood pH</p> Signup and view all the answers

Match the following components of acid-base chemistry with their definitions:

<p>Acid-Base Reaction = Involves transfer of H+ ions Neutral pH = Equal concentration of H+ and OH- Ocean Acidification = Decrease in ocean pH due to dissolved CO2 Calcification = Process of forming calcium carbonate, affected by carbonate concentration</p> Signup and view all the answers

Match the following pH values with their acidity levels:

<p>pH 3.0 = 1,000 times more acidic than pH 6.0 pH 7.0 = Neutral level close to blood pH pH 8.0 = Slightly basic, common for biological substances pH 5.0 = Acidic but not as strong as pH 3.0</p> Signup and view all the answers

Match the following Avogadro's number concepts with their explanations:

<p>1 Mole = Contains $6.02*10^{23}$ molecules 342 g of Sucrose = Contains the same number of molecules as 10 g of Substance B Molecular Mass = Total mass of all atoms in a molecule Dalton = Unit of measurement for atomic mass</p> Signup and view all the answers

Match the following types of molecules with their descriptions:

<p>Polar Molecules = Dissolve in water due to hydrogen bonding Nonpolar Molecules = Do not form hydrogen bonds with water Large Compounds = Absorb water even when not dissolving Ions = Form hydration shells when surrounded by water</p> Signup and view all the answers

Study Notes

Concept 2.1: Chemical Composition of Life

  • Elements are basic substances that cannot be broken down further, forming the building blocks of all matter.
  • Compounds are substances formed from two or more different bonded atoms.
  • Life requires 20-25% of the 92 naturally occurring elements.
    • Humans need 25 elements.
    • Plants need 17 elements.
  • Oxygen, carbon, hydrogen, and nitrogen make up 96% of living matter.
  • Calcium, phosphorus, potassium, and sulfur make up the remaining 4%.
  • Trace elements are present in small quantities in specific organisms.
  • Some naturally occurring elements are toxic, but organisms in these environments have evolved tolerance.

Concept 2.2: Atoms and Atomic Structure

  • Atoms are the smallest units of elements.

  • Subatomic particles include neutrons, protons, and electrons.

  • Protons (positive charge) and electrons (negative charge) are electrically charged.

  • Protons and neutrons are tightly packed into the atom's nucleus.

  • Electrons orbit the nucleus, forming a region of negative charge.

  • Atomic mass is measured in daltons.

    • Neutrons and protons have a mass of 1 Dalton.
    • Electrons have a significantly smaller mass (around 1/2000 of a Dalton), and are thus ignored in calculating atomic mass.
  • Atomic number = number of protons (usually equal to the number of electrons in a neutral atom).

  • Mass number = number of protons + number of neutrons.

  • Atomic mass = average mass of all isotopes of an element, a decimal value reflecting the relative abundance of isotopes.

  • Isotopes are atoms of the same element with differing numbers of neutrons.

  • Radioactive isotopes are unstable and release energy (e.g., heat) as their nuclei decay.

    • The decay can convert one element into another.
  • Radioactive tracers are used to track isotopes within organisms (e.g., PET scans).

  • Half-life refers to the time it takes for half of a radioactive isotope to decay.

  • Radiometric dating calculates the passage of half-lives since a fossil or rock formed.

  • Atoms are mostly empty space.

    • Electrons are involved in chemical reactions, not the nucleus.
  • Energy is the capacity to cause change.

  • Matter tends to move towards lower energy states (e.g., water flowing downhill).

  • Electrons exist in specific energy levels (electron shells) around the nucleus, determined by distance.

  • Energy absorption or release is required for electrons to move between electron shells.

  • A chemical's behavior is dependent on its electron configuration.

    • First shell holds 2 electrons, second shell holds 8
    • Valence shell (outermost shell) and valence electrons dictate chemical behavior.
  • Atoms with filled valence shells are largely unreactive.

  • Orbitals are regions where an electron is most likely to be found (90% probability).

  • The reactivity of an atom depends on the arrangement of unpaired electrons in its orbitals.

Concept 2.3: Chemical Bonds

  • Chemical bonds form when atoms with incomplete electron shells interact to achieve a filled outer shell.
  • Covalent bonds involve sharing electron pairs.
  • Lewis dot structures show electron distribution as dots (e.g., H:H).
  • Structural formulas use lines to represent bonds (e.g., H-H).
  • Double bonds involve the sharing of two pairs of electrons.
  • Valence is an atom's bonding capacity, determined by the number of electrons needed to fill its valence shell.
  • Electronegativity measures an atom's attraction for shared electrons.
  • Nonpolar covalent bonds form between atoms with similar electronegativity.
  • Polar covalent bonds form between atoms with different electronegativity; the bond is then polarized.
  • Ions are atoms that have gained or lost electrons.
  • Cations are positively charged ions, anions are negatively charged ions.
  • Ionic bonds form between oppositely charged ions.
  • Salts are ionic compounds formed from ionic bonds.
  • Ionic bonds are stronger in dry conditions but weaker when in solution.
  • Weak chemical interactions (e.g., hydrogen bonds, van der Waals) are crucial for molecular interactions in cells.
    • Hydrogen bonds involve a hydrogen atom bonded to an electronegative atom.
    • Van der Waals forces create temporary attractions between molecules.
  • Molecular shape influences interactions with other molecules.

Concept 2.4: Chemical Reactions

  • Chemical reactions involve bond formation and breaking.
  • Reactants produce products.
  • Mass is conserved in chemical reactions (atoms are rearranged).
  • Reversible reactions occur when products can reform reactants.
  • Reaction rates can be affected by reactant concentrations.
  • Chemical equilibrium occurs when the forward and reverse reaction rates are equal.

Concept 3.1: Properties of Water

  • Water's polarity results in hydrogen bonding, causing water molecules to attract each other.
  • Hydrogen bonds in liquid water are constantly forming and breaking.
  • Ice is less dense than liquid water due to hydrogen bonding in crystal structure.
  • Water exhibits polar covalent bonds.
  • Polarity describes molecules with unequal charge distributions.

Concept 3.2: Water's Unique Properties

  • Cohesion is the attraction between like molecules (e.g. water molecules).
  • Surface tension results from cohesion, creating a "skin".
  • Adhesion is the clinging of one substance to another different substance (e.g., water to plant cells).
  • High specific heat means water can absorb a substantial amount of heat before its temperature increases.
  • Water resists temperature change.
  • Hydrogen bonding is crucial to water's high specific heat, as breaking H-bonds requires considerable energy.

Concept 3.3: Water's Role as a Solvent

  • Water is an excellent solvent.
    • Water molecules surround dissolved substances leading to a hydration shell.
  • Hydrophilic substances dissolve in water.
  • Hydrophobic substances do not interact readily with water.

Additional Concepts

  • Matter terms: Kinetic Energy, thermal energy, temperature, heat, calorie, kilocalorie, joule, specific heat
  • Heat of vaporization describes energy needed to change liquid to gas.
  • Solutions involve solutes dissolved in solvents.
  • Molarity is a unit of concentration.
  • Molecules have an associated mass determined by summing constituent atomic masses.
  • Moles are a unit relating mass to the number of molecules (Avogadro's number).
  • pH is related to H+ concentration.
  • Buffers resist pH change and maintain homeostasis.
  • Ocean acidification is a consequence of increased CO2 leading to lower pH in the oceans.

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Explore the essential concepts of chemical composition that are fundamental to life. This quiz covers the elements crucial for living organisms, the structure of atoms, and the role of subatomic particles. Test your understanding of how these elements contribute to biological processes.

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