Chemistry Chapter: Matter and Atomic Structure 2.2
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Questions and Answers

What type of bond is responsible for the unique liquid properties of water?

  • Van der Waals interaction
  • Covalent bond
  • Ionic bond
  • Hydrogen bond (correct)

    • Which of the following is NOT a characteristic of van der Waals interactions?

  • They occur between polar molecules.
  • They are important in biological systems.
  • They are weak attractions between molecules.
  • They are caused by temporary partial charges.
  • They are responsible for the double-stranded structure of DNA. (correct)

    • How do hydrogen bonds hold together two long strands of DNA?

  • By forming bonds between the hydrogen atoms on one strand and the oxygen atoms on the other strand.
  • By creating a hydrophobic interaction between the two strands.
  • By attracting the negatively charged phosphate groups on one strand to the positively charged sugar molecules on the other strand.
  • By attracting the nitrogenous bases of one strand to the nitrogenous bases of the other strand. (correct)
  • By forming a temporary covalent bond between the two strands.

    • What is a key role played by radiography technologists in medical diagnosis?

    <p>Explaining medical procedures to patients. (A)</p> Signup and view all the answers

    Which imaging technique uses fluctuating magnetic fields to produce images?

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

    What is the main type of molecule that is targeted for MRI imaging?

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

    Why are hydrogen bonds essential for life?

    <p>They contribute to the unique properties of water, making it a suitable solvent for life. (D)</p> Signup and view all the answers

    What is the primary difference between X-ray and MRI imaging?

    <p>X-ray images bones, while MRI images soft tissues. (B)</p> Signup and view all the answers

    What is the role of a radiologist in the imaging process?

    <p>Analyzing the images and providing a diagnosis. (E)</p> Signup and view all the answers

    Which of the following is NOT a benefit of a mammogram?

    <p>Reduced risk of developing breast cancer. (B)</p> Signup and view all the answers

    Which of the following best describes the octet rule?

    <p>It explains the tendency of atoms to have eight electrons in their outermost shell to achieve stability. (C)</p> Signup and view all the answers

    What happens to an atom when it becomes an ion?

    <p>It loses electrons or gains electrons, resulting in a net charge. (D)</p> Signup and view all the answers

    What type of bond forms when sodium (Na) and chlorine (Cl) atoms react to form sodium chloride (NaCl)?

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

    Which of the following statements accurately describes a covalent bond?

    <p>Electrons are shared unequally between two atoms. (B)</p> Signup and view all the answers

    Which of the following is an example of a nonpolar covalent bond?

    <p>CH4 (methane) (A), O2 (oxygen) (B)</p> Signup and view all the answers

    Which of the following bonds is the weakest?

    <p>van der Waals (D)</p> Signup and view all the answers

    Which of the following is NOT a type of chemical bond?

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

    What is the main reason atoms form chemical bonds?

    <p>To achieve a stable electron configuration (D)</p> Signup and view all the answers

    Explain how the octet rule governs the formation of ionic bonds.

    <p>Atoms gain or lose electrons to achieve a full outer shell, resulting in oppositely charged ions that attract. (D)</p> Signup and view all the answers

    Which of the following is true regarding polar covalent bonds?

    <p>Electrons are shared unequally between two atoms, leading to a slight charge separation. (C)</p> Signup and view all the answers

    What is the difference between a cation and an anion?

    <p>A cation is a positively charged ion, while an anion is a negatively charged ion. (D)</p> Signup and view all the answers

    How does the formation of a covalent bond affect the stability of the participating atoms?

    <p>It increases the stability of the atoms by filling their outer shells, leading to a lower energy state. (B)</p> Signup and view all the answers

    Which of the following pairs of atoms would most likely form a polar covalent bond?

    <p>Hydrogen (H) and Oxygen (O) (B)</p> Signup and view all the answers

    What is the key difference between ionic and covalent bonds in terms of electron behavior?

    <p>Electrons are transferred in ionic bonds and shared in covalent bonds. (B)</p> Signup and view all the answers

    Give an example of a molecule that is held together by covalent bonds.

    <p>Water (H2O) (B), Carbon dioxide (CO2) (C), All of the above (D)</p> Signup and view all the answers

    What is the main reason why water is a polar molecule?

    <p>The oxygen atom is more electronegative than the hydrogen atoms, resulting in an uneven distribution of electrons. (D)</p> Signup and view all the answers

    What is the smallest unit of an element that retains the chemical properties of that element?

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

    Which of the following elements is NOT found naturally?

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

    Which subatomic particle carries a positive charge?

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

    Which of the following statements about atoms is true?

    <p>The number of protons in an atom determines its chemical properties. (D)</p> Signup and view all the answers

    Which of the following is a characteristic of neutrons?

    <p>They have a mass of 1. (D)</p> Signup and view all the answers

    Which of the following represents the correct hierarchy of organization in multicellular organisms, from smallest to largest?

    <p>Molecule - Cell - Tissue - Organ - Organism (A)</p> Signup and view all the answers

    What is the difference between an element and an atom?

    <p>An atom is the smallest unit of an element, while an element is a pure substance made up of atoms. (C)</p> Signup and view all the answers

    Which subatomic particle is responsible for the chemical properties of an element?

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

    Identify the isotope of carbon that is used to date fossils.

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

    Which element has the largest atomic number out of the following?

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

    What is the primary factor that determines how elements interact with one another?

    <p>The arrangement and number of electrons in the outermost shell (C)</p> Signup and view all the answers

    How many electrons can the second energy level hold?

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

    When an organism dies, the relative level of 14C in its body will ______ due to the decay of 14C to 14N.

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

    Which statement accurately describes isotopes?

    <p>Isotopes are atoms of the same element with different numbers of neutrons. (B)</p> Signup and view all the answers

    What is the mass number of an atom with 11 protons and 12 neutrons?

    <p>23 (A)</p> Signup and view all the answers

    Why are the elements arranged in rows on the periodic table?

    <p>They have the same number of electron shells. (D)</p> Signup and view all the answers

    Which of the following is NOT a characteristic of radioactive isotopes?

    <p>They are always stable. (B)</p> Signup and view all the answers

    What is the main difference between Carbon-12 and Carbon-14?

    <p>Carbon-12 has 6 protons and 6 neutrons, while Carbon-14 has 6 protons and 8 neutrons. (D)</p> Signup and view all the answers

    The time it takes for half of the original concentration of a radioactive isotope to decay is called its ___?

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

    Why is it important to understand the number of electrons in the outer shell of an atom?

    <p>It determines how the atom will bond with other atoms. (A)</p> Signup and view all the answers

    What is the maximum number of electrons that can occupy the first energy level of an atom?

    <p>2 (D)</p> Signup and view all the answers

    What is the main reason why scientists use isotopes like Carbon-14 to date fossils?

    <p>Carbon-14 decays at a constant rate, providing a reliable time marker. (C)</p> Signup and view all the answers

    What is the most common isotope of carbon?

    <p>Carbon-12 (B)</p> Signup and view all the answers

    The arrangement of the periodic table shows the relationship between an element's ________ and its ________.

    <p>atomic number, electron configuration (A)</p> Signup and view all the answers

    Flashcards

    Matter

    Anything that occupies space and has mass.

    Element

    A substance that cannot be broken down chemically into simpler substances.

    Atom

    The smallest unit of an element that retains its properties.

    Chemical Symbol

    A one- or two-letter notation for an element (e.g., H, O, Na).

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    Proton

    A positively charged particle found in the nucleus of an atom.

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    Electron

    A negatively charged particle that orbits the nucleus.

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    Neutron

    A particle in the nucleus with no charge and mass equivalent to protons.

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    Isotope

    Atoms of the same element with different numbers of neutrons.

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    Chemical Bonds

    Interactions that form molecules by atoms connecting.

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    Octet Rule

    Atoms tend to fill their outer shells with eight electrons for stability.

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    Ions

    Atoms with unequal numbers of protons and electrons, leading to a net charge.

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    Cations

    Positive ions formed by losing electrons.

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    Anions

    Negative ions formed by gaining electrons.

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    Electron Transfer

    The movement of electrons from one atom to another during bonding.

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    Ionic Bond

    A bond formed between oppositely charged ions via electron transfer.

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    Covalent Bond

    A bond formed by sharing electrons between atoms.

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    Polar Covalent Bond

    A bond where electrons are shared unequally, creating slight charges.

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    Nonpolar Covalent Bond

    A bond where electrons are shared equally between atoms.

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    Water (H2O) Bonding

    Covalent bonds forming water, with oxygen pulling electron density closer.

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    Triple Covalent Bond

    A strong bond involving three shared electrons between atoms.

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    Methane (CH4) Bonding

    Covalent bonding of carbon with four hydrogen atoms, equal sharing.

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    Hydrogen Bonds

    Weak attractions between polar molecules, like between water molecules.

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    Van der Waals Interactions

    Weak attractions between molecules or parts of molecules.

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    Unique Properties of Water

    Features like high boiling point and solvent abilities due to hydrogen bonding.

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    DNA Structure

    The double-stranded shape of DNA is maintained by hydrogen bonds between bases.

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    Magnetic Resonance Imaging (MRI)

    A technique using magnetic fields to create images of soft tissues.

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    Radiography Technician

    A professional who produces images for medical examination using radiological techniques.

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    Electronegativity

    The ability of an atom to attract shared electrons in a bond.

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    Partial Charge

    A charge that occurs when electrons are unequally shared in a bond, creating polarity.

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    Soft Tissues in Imaging

    Body tissues like muscles and organs that MRI can capture images of.

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    Mass of an atom

    The total mass determined by the number of protons and neutrons.

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    Atomic number

    The number of protons in an atom that defines the element.

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    Mass number

    Total number of protons plus neutrons in an atom.

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    Determining neutrons

    The number of neutrons equals mass number minus atomic number.

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    Periodic table

    A chart organizing elements based on atomic number and properties.

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    Radioactive isotopes

    Isotopes that decay into more stable forms over time.

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    Carbon-14

    A radioactive isotope of carbon used in dating fossils.

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    Half-life

    The time it takes for half of a sample of an isotope to decay.

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    Electron shells

    Energy levels around the nucleus where electrons reside.

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    Valence electrons

    Electrons in the outermost shell that determine reactivity.

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    Stable atom

    An atom with a full outer electron shell.

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    Elements in the first row

    Hydrogen and helium, with only the first shell occupied.

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    Chemical bonding

    The process by which atoms combine based on electron arrangement.

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    Neon

    An element with a full outer shell of electrons, making it stable.

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    Study Notes

    Matter and Life

    • Life is fundamentally composed of matter, which occupies space and has mass.
    • Matter is made up of elements, substances that cannot be broken down chemically.
    • Currently, 118 elements are defined, with 92 occurring naturally and fewer than 30 found in living cells.
    • Elements are designated by chemical symbols (e.g., H, N, O, C, Na) and have unique properties.
    • Atoms are the smallest units of an element, retaining its chemical properties.
    • Atoms cannot be broken down into smaller parts without losing their elemental identity.

    Atomic Structure

    • Atoms consist of protons, electrons, and neutrons.
    • Protons are positively charged, located in the nucleus, with a mass of 1 and a charge of +1.
    • Electrons are negatively charged, outside the nucleus, with negligible mass and a charge of -1.
    • Neutrons are neutrally charged, located in the nucleus, with a mass of 1.
    • In a neutral atom, the number of protons equals the number of electrons.
    • Atomic mass is the sum of protons and neutrons.

    Isotopes

    • Isotopes are different forms of the same element with the same number of protons but different numbers of neutrons.
    • Carbon-12 and Carbon-14 are examples of carbon isotopes.
    • Radioactive isotopes (e.g., Carbon-14) are unstable and decay over time.
    • Half-life is the time it takes for half of a sample of a radioactive isotope to decay.
    • Carbon-14 dating is used to estimate the age of organic materials.

    Electron Arrangement and Shells

    • Electrons exist in energy levels (shells) surrounding the nucleus.
    • The closest shell holds a maximum of two electrons.
    • The second and third shells can hold a maximum of eight electrons each.
    • The arrangement of electrons determines how elements interact.
    • Elements with complete outermost electron shells are more stable.

    Chemical Bonds

    • Chemical bonds are interactions between elements creating molecules.
    • The octet rule states that atoms tend to gain, lose, or share electrons to achieve a complete outer shell (8 electrons).
    • Ions are atoms with unequal numbers of protons and electrons.
    • Cations are positively charged ions (formed by losing electrons).
    • Anions are negatively charged ions (formed by gaining electrons).
    • Electron transfer creates ionic bonds, where oppositely charged ions attract.
    • Covalent bonds form when atoms share electrons.

    Types of Covalent Bonds

    • Nonpolar covalent bonds: electrons shared equally.
    • Polar covalent bonds: electrons shared unequally, creating partial charges.
    • Hydrogen bonds are weak attractions between a slightly positive hydrogen atom and a slightly negative atom in another molecule.
    • Van der Waals interactions are weak attractions between molecules due to temporary fluctuations in electron distribution.

    Applications of Isotopes in Medicine

    • Medical imaging techniques use radioactive isotopes to visualize internal body structures (e.g., MRI, X-rays).

    Periodic Table

    • The periodic table organizes elements based on their properties.
    • The table shows atomic number, relative atomic mass, and electron arrangement.

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    Description

    Explore the fundamental concepts of matter and atomic structure in this quiz. Understand how matter is composed of elements and how atoms are structured with protons, neutrons, and electrons. Test your knowledge on the properties of the elements and the structure of atoms.

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