Chemistry Basics Quiz
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Questions and Answers

Which ion is formed when magnesium loses two electrons?

  • Mg-
  • Mg3+
  • Mg2+ (correct)
  • Mg+

    • What characterizes a free radical?

  • It has a stable outer shell of electrons.
  • It contains at least one unpaired electron. (correct)
  • It tends to be non-reactive with other molecules.
  • It is a molecule with a completely filled outer shell.

    • How does the shape of a molecule change?

  • Only through the breaking of bonds.
  • By rigidly maintaining bond angles.
  • Through rotation around single covalent bonds. (correct)
  • By losing or gaining electrons.

    • Which of the following ions is formed by chlorine when it gains an electron?

    <p>Cl-</p> Signup and view all the answers

    Which of the following statements is TRUE regarding potassium ions?

    <p>Potassium loses one electron to form K+.</p> Signup and view all the answers

    What is the smallest functional unit of matter that forms all chemical substances?

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

    Which of the following subatomic particles is positively charged?

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

    In the atomic model, where are electrons most likely to be found?

    <p>In defined orbitals</p> Signup and view all the answers

    How many electrons can the first electron shell hold?

    <p>2 electrons</p> Signup and view all the answers

    What are the electrons in the outer shell of an atom called?

    <p>Valence electrons</p> Signup and view all the answers

    What shape is a p orbital?

    <p>Dumbbell-shaped</p> Signup and view all the answers

    What is the maximum number of electrons that can be held in the second shell of an atom?

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

    Which of the following statements about atoms is correct?

    <p>The number of neutrons in an atom can vary.</p> Signup and view all the answers

    What do we call the representation of bonded pairs of electrons?

    <p>Lewis Structure</p> Signup and view all the answers

    Which two subatomic particles are found in the atomic nucleus?

    <p>Protons and Neutrons</p> Signup and view all the answers

    What causes a person's weight to change when moving from Earth to the Moon?

    <p>The gravitational pull on the person varying based on location</p> Signup and view all the answers

    What does one Dalton (Da) represent in atomic mass measurements?

    <p>1/12 the mass of a carbon atom</p> Signup and view all the answers

    Which of the following elements is NOT among the most abundant in living organisms?

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

    What is meant by the term 'isotope'?

    <p>Multiple forms of an element that differ in the number of neutrons</p> Signup and view all the answers

    What role do radioisotopes play in medicine?

    <p>They help in imaging and cancer treatment.</p> Signup and view all the answers

    What is Avogadro’s number used to define?

    <p>The number of atoms in a mole of any element</p> Signup and view all the answers

    Which of these elements is primarily found in proteins?

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

    Why are trace elements significant for organisms?

    <p>They are essential for normal growth and function despite their small quantities.</p> Signup and view all the answers

    Which statement accurately describes the difference between mass and weight?

    <p>Mass is the same regardless of location, while weight can change.</p> Signup and view all the answers

    What is a characteristic feature of a covalent bond?

    <p>Electrons are shared between atoms.</p> Signup and view all the answers

    How is a polar covalent bond different from a nonpolar covalent bond?

    <p>Polar bonds share electrons unequally between atoms of different electronegativities.</p> Signup and view all the answers

    What is the octet rule pertaining to atomic stability?

    <p>Atoms are stable when their outer shell contains 8 electrons.</p> Signup and view all the answers

    What type of bond is formed when a hydrogen atom from one molecule is attracted to an electronegative atom of another molecule?

    <p>Hydrogen bond</p> Signup and view all the answers

    Which of the following best describes ionic bonds?

    <p>They result from the attraction between positively and negatively charged ions.</p> Signup and view all the answers

    What happens during the formation of van der Waals dispersion forces?

    <p>Electrons create a fleeting electrical attraction between molecules.</p> Signup and view all the answers

    What distinguishes a cation from an anion?

    <p>A cation has lost electrons, resulting in a positive charge.</p> Signup and view all the answers

    Which of the following is a true statement about molecular formulas?

    <p>The subscript indicates how many of each type of atom are present in a molecule.</p> Signup and view all the answers

    Which of the following statements about hydrogen bonds is correct?

    <p>Hydrogen bonds can form and break easily, but many can collectively provide strength.</p> Signup and view all the answers

    What is a defining characteristic of compounds compared to individual elements?

    <p>The properties of a compound can be drastically different than those of its individual elements.</p> Signup and view all the answers

    What distinguishes one element from another?

    <p>Number of protons</p> Signup and view all the answers

    What is the atomic number of an element equal to?

    <p>Number of protons in the nucleus</p> Signup and view all the answers

    How are elements organized in the periodic table?

    <p>By atomic number</p> Signup and view all the answers

    What determines the similar properties of elements within a column of the periodic table?

    <p>The number of outer shell electrons</p> Signup and view all the answers

    What is the relative mass of a neutron compared to an electron?

    <p>About 1,836 times that of an electron</p> Signup and view all the answers

    Which statement is true regarding the most common form of carbon?

    <p>It has six protons and six neutrons</p> Signup and view all the answers

    What does atomic mass indicate about an atom?

    <p>Its mass relative to other atoms</p> Signup and view all the answers

    Which of the following statements about protons is correct?

    <p>They reside in the nucleus.</p> Signup and view all the answers

    What is the ion symbol for the calcium ion after it loses its electrons?

    <p>Ca2+</p> Signup and view all the answers

    Which of the following bonds allows for the rotation of molecules due to its non-rigid nature?

    <p>Covalent bonds</p> Signup and view all the answers

    What typically causes the formation of free radicals?

    <p>Exposure to radiation and toxins</p> Signup and view all the answers

    Which element forms an ion with a single electron lost from its outer shell?

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

    How many electrons does potassium typically lose to form its ion?

    <p>1</p> Signup and view all the answers

    What is the total number of electrons that the second electron shell can hold?

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

    Which statement is correct regarding the structure of an atom?

    <p>Protons and electrons are found in equal numbers.</p> Signup and view all the answers

    What describes the arrangement of electrons in an atom?

    <p>Electrons exist in a cloud-like formation around the nucleus.</p> Signup and view all the answers

    What term is used to describe electrons that are available to form bonds with other atoms?

    <p>Valence electrons</p> Signup and view all the answers

    Which of the following statements is true regarding orbitals?

    <p>Each type of orbital can only hold a pair of electrons.</p> Signup and view all the answers

    What defines a chemical element?

    <p>Atoms with a specified number of protons.</p> Signup and view all the answers

    Which particle is NOT found in the nucleus of an atom?

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

    What are the shapes of the orbitals found in the second electron shell?

    <p>One spherical and three dumbbell-shaped</p> Signup and view all the answers

    What is the primary characteristic of a Lewis structure?

    <p>It depicts bonded pairs as lines.</p> Signup and view all the answers

    What differentiates the three states of matter?

    <p>Physical arrangement and energy of particles.</p> Signup and view all the answers

    What is the primary factor that distinguishes one element from another?

    <p>Number of protons</p> Signup and view all the answers

    When is the atomic number of an atom defined?

    <p>When it is determined by the number of protons</p> Signup and view all the answers

    What does the periodic table indicate about the columns of elements?

    <p>They indicate the number of valence electrons in the outer shell</p> Signup and view all the answers

    How does the atomic mass of an atom relate to protons and neutrons?

    <p>It is the combined mass of protons and neutrons</p> Signup and view all the answers

    What is the relative mass of a proton compared to an electron?

    <p>It is more than 1,800 times the mass of an electron</p> Signup and view all the answers

    Which statement accurately represents atomic mass in the context of different elements?

    <p>Carbon’s most common form has an atomic mass of exactly 12</p> Signup and view all the answers

    What does it mean when an atom has a net charge of zero?

    <p>The number of protons equals the number of electrons</p> Signup and view all the answers

    What is the role of neutrons in the atomic nucleus?

    <p>They have no charge and contribute to atomic mass</p> Signup and view all the answers

    What remains constant for a person regardless of their location in the universe?

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

    Which of these elements constitutes the highest percentage of human body mass?

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

    What is the primary function of mineral elements in living organisms?

    <p>Essential for normal growth and function</p> Signup and view all the answers

    What defines isotopes of an element?

    <p>They have different numbers of neutrons.</p> Signup and view all the answers

    What is one Dalton equivalent to in atomic mass measurements?

    <p>1/12 the mass of a carbon atom</p> Signup and view all the answers

    Which of the following correctly describes Avogadro's number?

    <p>It is the number of atoms in one mole of any element.</p> Signup and view all the answers

    Which among the following elements is classified as a trace element?

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

    Which of the following statements regarding radioactive isotopes is correct?

    <p>They emit radiation as they decay.</p> Signup and view all the answers

    Which combination of elements makes up about 95% of the atoms in living organisms?

    <p>Carbon, Oxygen, Hydrogen, and Nitrogen</p> Signup and view all the answers

    What is the common atomic mass of a carbon atom?

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

    What role do antioxidants play in the body?

    <p>They donate electrons without becoming highly reactive.</p> Signup and view all the answers

    What is a key property of water that allows it to dissolve various substances?

    <p>It is a polar molecule.</p> Signup and view all the answers

    Which type of molecules do not dissolve in water?

    <p>Hydrophobic molecules</p> Signup and view all the answers

    What property of water contributes to its high specific heat?

    <p>Hydrogen bonding between water molecules.</p> Signup and view all the answers

    Which solution would be classified as acidic?

    <p>pH 5</p> Signup and view all the answers

    What is the effect of adding solutes to water?

    <p>It lowers both the freezing point and boiling point.</p> Signup and view all the answers

    What does molarity measure?

    <p>The concentration of a solute in a solution.</p> Signup and view all the answers

    Why is water considered an excellent solvent?

    <p>Because of its polar characteristics which allow hydrogen bonding.</p> Signup and view all the answers

    What happens to the shape and function of molecules in relation to pH?

    <p>pH can alter molecular shapes and consequently their functions.</p> Signup and view all the answers

    What is the primary action of buffers in biological systems?

    <p>Maintain a constant pH despite fluctuations.</p> Signup and view all the answers

    Which of the following compounds is considered an amphipathic molecule?

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

    What defines colligative properties of water?

    <p>They depend on the total number of dissolved solute particles.</p> Signup and view all the answers

    What is the primary function of water in living organisms?

    <p>It participates in various chemical reactions.</p> Signup and view all the answers

    Study Notes

    Magnesium Ion

    • Magnesium forms a Mg²⁺ ion when it loses two electrons.

    Free Radicals

    • A free radical is an atom or molecule with an unpaired electron.

    Molecular Shape Change

    • The shape of a molecule can change based on the interactions of its constituent atoms.
      • This is due to the positioning of the electron pairs forming the chemical bonds, as well as lone pairs of electrons.

    Chlorine Ion

    • When chlorine gains an electron, it forms the Cl⁻ ion.

    Potassium Ions

    • Potassium ions (K⁺) carry a positive charge, are essential for nerve function, and are involved in muscle contractions.

    Smallest Functional Unit of Matter

    • The atom is the smallest unit of matter that can exist in a free state. It can not be broken down by chemical means.

    Positively Charged Subatomic Particle

    • The proton is a positively charged subatomic particle.

    Electron Location

    • In the atomic model, electrons are most likely to be found in electron shells or orbitals surrounding the nucleus.

    First Electron Shell Capacity

    • The first electron shell can hold a maximum of two electrons.

    Outer Shell Electrons

    • Electrons in the outer shell of an atom are called valence electrons.

    P Orbital Shape

    • P orbitals have a dumbbell shape.

    Second Electron Shell Capacity

    • The second electron shell can hold up to eight electrons.

    Atomic Structure

    • Atoms are made up of protons, neutrons, and electrons and are mostly empty space.

    Electron Pair Representation

    • We call the representation of bonded pairs of electrons a Lewis structure.

    Subatomic Particles in the Nucleus

    • Protons and neutrons are found in the atomic nucleus.

    Weight Change on the Moon

    • A person's weight changes from Earth to the Moon due to the difference in gravity between the two celestial bodies.

    Dalton (Da)

    • One Dalton (Da) represents the average mass of one proton or neutron.

    Least Abundant Element

    • The least abundant element among those found in living organisms is iron (Fe).

    Isotopes

    • Isotopes are atoms of the same element that have the same number of protons but differ in the number of neutrons.

    Radioisotopes in Medicine

    • Radioisotopes are used in medicine for diagnosis and treatment.
      • They can be used, for example, to image and treat cancer.
      • They can also be used to sterilize medical equipment.

    Avogadro's Number

    • Avogadro's number (6.022 x 10²³) defines the number of atoms or molecules present in one mole of a substance.

    Element Primarily Found in Proteins

    • Nitrogen (N) is the element primarily found in proteins.

    Significance of Trace Elements

    • Trace elements are essential for life, even in small amounts, as they play crucial roles in various biological processes.

    Mass vs. Weight

    • Mass is the amount of matter in an object, while weight is the force exerted on an object due to gravity.

    Covalent Bond Characteristic

    • Covalent bonds are formed by the sharing of electrons between two atoms.

    Polar vs. Nonpolar Covalent Bond

    • In polar covalent bonds, electrons are shared unequally between atoms, creating a partial positive and partial negative charge.
    • In nonpolar covalent bonds, electrons are shared equally, resulting in no charge difference.

    Octet Rule

    • The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable configuration of eight electrons in their outermost shell.

    Hydrogen Bonds

    • Hydrogen bonds are formed when a hydrogen atom covalently linked to a highly electronegative atom is attracted to a lone pair of electrons in another electronegative atom.

    Ionic Bonds

    • Ionic bonds are formed by the electrostatic attraction between oppositely charged ions.

    Van Der Waals Dispersion Forces

    • Van der Waals dispersion forces are weak, temporary attractions between nonpolar molecules caused by temporary fluctuations in electron distribution.

    Cation vs. Anion

    • Cations are positively charged ions that are formed when an atom loses electrons.
    • Anions are negatively charged ions that are formed when an atom gains electrons.

    Molecular Formulas

    • Molecular formulas indicate the types and numbers of each atom in a molecule.

    Hydrogen Bonds

    • Hydrogen bonds are weak attractions between molecules, but they are important for many biological processes.

    Compounds vs. Elements

    • Compounds involve two or more elements chemically combined in a fixed ratio.
    • Elements are pure substances consisting of only one type of atom.

    Distinguishing Elements

    • Elements are distinguished from one another by their atomic number, which is equal to the number of protons in their nucleus.

    Atomic Number

    • The atomic number of an element is equal to the number of protons in its nucleus.

    Periodic Table Organization

    • Elements in the periodic table are organized by increasing atomic number.

    Periodic Table Columns

    • Elements within a column (group) of the periodic table have similar properties due to having the same number of valence electrons.

    Neutron Mass

    • The relative mass of a neutron is about 1 (slightly larger than a proton).
      • In comparison, the mass of an electron is negligible.

    Common Form of Carbon

    • Carbon-12 (¹²C) is the most common form of carbon, containing six protons and six neutrons.

    Atomic Mass

    • Atomic mass indicates the average weight of an atom of an element. It is primarily determined by the number of protons and neutrons in the nucleus.

    Protons

    • Protons are positively charged subatomic particles found in the nucleus of an atom.

    Calcium Ion Symbol

    • The ion symbol for the calcium ion after it loses its electrons is Ca²⁺.

    Bond Allowing Molecular Rotation

    • Single bonds are typically non-rigid, allowing for free rotation of attached molecules.

    Free Radical Formation

    • Free radicals often form because of the presence of unstable, unpaired electrons due to factors like UV light, chemical reactions, or metabolic processes.

    Element Losing One Electron

    • Sodium (Na) is an element that forms an ion with a single electron lost from its outer shell, resulting in Na⁺.

    Electrons Lost by Potassium

    • Potassium (K) typically loses one electron to form its ion, K⁺.

    Second Shell Electron Capacity

    • The second electron shell can hold up to eight electrons.

    Atomic Structure Description

    • Atoms consist of a nucleus containing protons and neutrons, surrounded by a cloud of electrons in specific energy levels.

    Electron Arrangement in Atom

    • The arrangement of electrons in an atom is described by its electronic configuration.

    Bonding Electrons

    • Electrons that are available to form bonds with other atoms are called valence electrons.

    Orbitals

    • Orbitals are three-dimensional regions around the nucleus where electrons are most likely to be found.

    Chemical Element Definition

    • A chemical element is a pure substance that cannot be broken down into simpler substances by chemical means.

    Particle Not in the Nucleus

    • Electrons are not found in the nucleus of an atom.

    Second Shell Orbital Shapes

    • The second electron shell contains one s orbital (spherical shape) and three p orbitals (dumbbell shape).

    Lewis Structure Characteristic

    • Lewis structures represent the bonding between atoms in a molecule by showing the valence electrons.

    Matter States

    • The three states of matter (solid, liquid, and gas) are differentiated by the degree of movement and arrangement of their constituent particles.

    Element Distinguishing Factor

    • The number of protons in the nucleus of an atom defines its atomic number and therefore distinguishes one element from another.

    Atomic Number Definition

    • The atomic number of an atom is defined by the number of protons in its nucleus.

    Periodic Table Columns

    • The columns of elements in the periodic table represent groups of elements with similar chemical properties due to the same number of valence electrons.

    Atomic Mass

    • Atomic mass of an atom is approximately equal to the total number of protons and neutrons in its nucleus.

    Proton Mass

    • The relative mass of a proton is about 1.
      • In comparison, the mass of an electron is negligible.
      • One atomic mass unit (amu) is approximately equal to the mass of a proton or a neutron.

    Atomic Mass Representation

    • Atomic mass represents the average weight of an atom of an element, taking into account the relative abundance of its isotopes.

    Net Charge of Zero

    • An atom with a net charge of zero means that the number of protons (positive charge) is equal to the number of electrons (negative charge).

    Neutron Role

    • Neutrons in the atomic nucleus contribute to the atom's mass and influence its stability.

    Constant for a Person

    • Mass remains constant for a person regardless of their location in the universe.

    Human Body Mass Percentage

    • Oxygen (O) constitutes the highest percentage of human body mass.

    Mineral Element Function

    • Mineral elements play essential roles in biological processes, including structural support, nerve function, and maintaining fluid balance.

    Defining Isotopes

    • Isotopes of an element are atoms that have the same number of protons but differ in the number of neutrons.

    Dalton Equivalence

    • 1 Dalton (Da) is equivalent to 1 atomic mass unit (amu).

    Avogadro's Number Description

    • Avogadro's number (6.022 x 10²³) represents the number of atoms or molecules present in one mole of a substance.

    Trace Element

    • Iron (Fe) is classified as a trace element.

    Radioactive Isotopes

    • Radioactive isotopes are unstable isotopes that undergo radioactive decay, emitting radiation.

    Abundant Elements in Living Organisms

    • Carbon (C), hydrogen (H), oxygen (O), and nitrogen (N) make up approximately 95% of the atoms in living organisms.

    Carbon Atomic Mass

    • The common atomic mass of a carbon atom is 12 atomic mass units (amu).

    Antioxidant Function

    • Antioxidants protect cells from damage caused by free radicals.

    Water's Dissolving Property

    • Water's polarity allows for the formation of hydrogen bonds, enabling it to dissolve various substances, especially polar or ionic compounds.

    Molecules Insoluble in Water

    • Nonpolar molecules, like fats and oils, do not dissolve well in water.

    High Specific Heat Property

    • Water's high specific heat is due to the strong hydrogen bonds between water molecules, requiring a significant amount of energy to raise its temperature.

    Acidic Solution

    • A solution with a pH less than 7 is classified as acidic.

    Solutes and Water

    • Adding solutes to water will increase its density and lower its freezing point.

    Molarity

    • Molarity measures the concentration of a solution, indicating the number of moles of solute dissolved per liter of solution.

    Water as a Solvent

    • Water is an excellent solvent due to its high polarity, which allows it to form hydrogen bonds with polar and ionic compounds.

    pH and Molecule Shape/Function

    • Changes in pH can alter the shape and function of molecules by affecting the interactions of hydrogen atoms and charged groups.

    Biological Buffers

    • Buffers in biological systems help maintain a stable pH by neutralizing the addition of acids or bases.

    Amphipathic Molecule

    • An amphipathic molecule has both hydrophilic (water-loving) and hydrophobic (water-fearing) regions.
      • An example is a phospholipid.

    Colligative Properties

    • Colligative properties of water are properties that depend on the concentration of solute particles present, not their specific identity.
      • Examples include lowering the freezing point and raising the boiling point.

    Water's Function

    • Water plays a crucial role in all living organisms as a solvent, reactant in chemical reactions, and a component of cells and tissues.

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