Podcast
Questions and Answers
What is the pH range of a solution that is considered acidic?
What is the pH range of a solution that is considered acidic?
- 0 to 6 (correct)
- 1 to 7
- 7 to 14
- 6 to 10
A solution with a pH of 10 is how many times more acidic than a solution with a pH of 12?
A solution with a pH of 10 is how many times more acidic than a solution with a pH of 12?
- 10 times
- 1000 times
- 100 times (correct)
- 10,000 times
Which of the following is NOT a characteristic of a buffer?
Which of the following is NOT a characteristic of a buffer?
- A buffer helps maintain a stable pH.
- A buffer can prevent significant pH changes when either an acid or a base is added.
- A buffer can only prevent pH changes when an acid is added. (correct)
- A buffer can be a single substance or a group of substances.
What is the difference between a colloid and a suspension?
What is the difference between a colloid and a suspension?
Which of the following is an example of a colloid?
Which of the following is an example of a colloid?
What is the pH of a neutral solution?
What is the pH of a neutral solution?
What happens during neutralization?
What happens during neutralization?
A strong base is characterized by:
A strong base is characterized by:
Which of the following is NOT a characteristic of electrolytes?
Which of the following is NOT a characteristic of electrolytes?
What is the reason why hydrophobic substances do not dissolve in water?
What is the reason why hydrophobic substances do not dissolve in water?
What is the term used to describe the interaction between nonpolar molecules that are excluded from water?
What is the term used to describe the interaction between nonpolar molecules that are excluded from water?
Which of the following is TRUE about amphipathic molecules?
Which of the following is TRUE about amphipathic molecules?
What is the term used to describe the ion formed when a water molecule gains a hydrogen ion?
What is the term used to describe the ion formed when a water molecule gains a hydrogen ion?
What is the difference between a strong acid and a weak acid?
What is the difference between a strong acid and a weak acid?
What is the term used to describe a substance that accepts protons when added to a solution?
What is the term used to describe a substance that accepts protons when added to a solution?
Which of the following substances is an example of an electrolyte?
Which of the following substances is an example of an electrolyte?
What structural feature gives elasticity to fibrous proteins found in skin or hair?
What structural feature gives elasticity to fibrous proteins found in skin or hair?
Which of the following describes the primary distinction between fibrous and globular proteins?
Which of the following describes the primary distinction between fibrous and globular proteins?
What is required for the normal function of some proteins, as exemplified by heme in hemoglobin?
What is required for the normal function of some proteins, as exemplified by heme in hemoglobin?
Which structure is characterized by the arrangement of two or more polypeptide chains?
Which structure is characterized by the arrangement of two or more polypeptide chains?
What typically occurs to a protein when it undergoes denaturation?
What typically occurs to a protein when it undergoes denaturation?
Which type of protein is likely to exhibit a compact, spherical shape?
Which type of protein is likely to exhibit a compact, spherical shape?
What effect does an improper pH have on proteins?
What effect does an improper pH have on proteins?
The biological activity of proteins is disturbed when which condition is met?
The biological activity of proteins is disturbed when which condition is met?
Which property of water is responsible for its ability to form beads on a surface?
Which property of water is responsible for its ability to form beads on a surface?
What is the specific heat of water primarily attributed to?
What is the specific heat of water primarily attributed to?
What does the heat of vaporization refer to in the context of water?
What does the heat of vaporization refer to in the context of water?
Which term describes substances that do not dissolve in water?
Which term describes substances that do not dissolve in water?
How does temperature affect the kinetic energy of water molecules?
How does temperature affect the kinetic energy of water molecules?
What is the relationship between water's polarity and its ability to dissolve substances?
What is the relationship between water's polarity and its ability to dissolve substances?
Which phase of water has the highest energy and molecular movement?
Which phase of water has the highest energy and molecular movement?
What role does adhesion play in the interactions of water with other substances?
What role does adhesion play in the interactions of water with other substances?
What is defined as a substance that has mass and occupies space?
What is defined as a substance that has mass and occupies space?
Which of the following is the smallest particle that exhibits the chemical properties of an element?
Which of the following is the smallest particle that exhibits the chemical properties of an element?
Which of the following elements is the largest and heaviest naturally occurring element?
Which of the following elements is the largest and heaviest naturally occurring element?
What are the three subatomic particles that compose an atom?
What are the three subatomic particles that compose an atom?
Which particle is uncharged and has a mass of 1 atomic mass unit (amu)?
Which particle is uncharged and has a mass of 1 atomic mass unit (amu)?
What distinguishes protons from neutrons?
What distinguishes protons from neutrons?
Where are electrons located in an atom?
Where are electrons located in an atom?
Which of the following elements is not categorized as a major element in the human body?
Which of the following elements is not categorized as a major element in the human body?
What defines a hydrogen bond?
What defines a hydrogen bond?
Which molecules are involved in hydrophobic interactions?
Which molecules are involved in hydrophobic interactions?
What type of molecules make up water?
What type of molecules make up water?
Why does water have a polar nature?
Why does water have a polar nature?
How many hydrogen bonds can one water molecule form with adjacent molecules?
How many hydrogen bonds can one water molecule form with adjacent molecules?
What is an example of intramolecular attraction?
What is an example of intramolecular attraction?
What happens to nonpolar atoms when electrons are distributed unequally?
What happens to nonpolar atoms when electrons are distributed unequally?
What are organic molecules defined as?
What are organic molecules defined as?
Flashcards
Hydrogen Bond
Hydrogen Bond
A weak attraction between a partially positive hydrogen atom and a partially negative atom in another molecule.
Polar Molecule
Polar Molecule
A molecule with an unequal distribution of charge, leading to partial positive and negative ends.
Nonpolar Molecule
Nonpolar Molecule
A molecule that has an equal distribution of charge, with no positive or negative poles.
Hydrophobic Interactions
Hydrophobic Interactions
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Intramolecular Attractions
Intramolecular Attractions
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Intermolecular Attractions
Intermolecular Attractions
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Electronegativity
Electronegativity
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Molecular Structure of Water
Molecular Structure of Water
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Atom
Atom
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Subatomic Particles
Subatomic Particles
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Periodic Table
Periodic Table
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Element
Element
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Major Elements
Major Elements
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Neutron
Neutron
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Electron
Electron
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Atomic Mass Unit (amu)
Atomic Mass Unit (amu)
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Phases of water
Phases of water
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Functions of water in the body
Functions of water in the body
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Cohesion
Cohesion
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Surface tension
Surface tension
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Adhesion
Adhesion
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Specific heat
Specific heat
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Heat of vaporization
Heat of vaporization
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Hydrophilic substances
Hydrophilic substances
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pH scale
pH scale
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Neutral pH
Neutral pH
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Acidic solution
Acidic solution
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Basic solution
Basic solution
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10-fold change
10-fold change
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Neutralization
Neutralization
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Buffer
Buffer
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Types of water mixtures
Types of water mixtures
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Alpha Helix
Alpha Helix
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Beta-Pleated Sheet
Beta-Pleated Sheet
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Tertiary Structure
Tertiary Structure
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Fibrous Proteins
Fibrous Proteins
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Globular Proteins
Globular Proteins
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Quaternary Structure
Quaternary Structure
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Prosthetic Group
Prosthetic Group
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Denaturation
Denaturation
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Hydration Shell
Hydration Shell
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Dissociation in Water
Dissociation in Water
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Electrolytes
Electrolytes
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Nonelectrolytes
Nonelectrolytes
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Amphipathic Molecules
Amphipathic Molecules
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Hydronium Ion
Hydronium Ion
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Acid Definition
Acid Definition
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Study Notes
Atomic Structure
- Matter is defined as a substance that has mass and occupies space.
- Matter exists in three states: solid, liquid, and gas.
- Matter is composed of atoms.
- An atom is the smallest particle that exhibits an element's chemical properties.
- There are 92 naturally occurring elements.
- Hydrogen is the smallest and uranium is the largest and heaviest naturally occurring element.
- Ultraheavy elements larger than uranium have been produced.
- Elements are organized on the periodic table.
- Elements are grouped as major, minor, and trace elements based on their percentage in the human body.
- The most abundant elements in the human body are oxygen, carbon, hydrogen, nitrogen, calcium, phosphorus, sulfur, potassium, sodium, chlorine, magnesium, and iron.
- Atoms are composed of three subatomic particles: protons, neutrons, and electrons.
- Subatomic particles are differentiated by mass and charge.
- Neutrons are uncharged, with a mass of 1 atomic mass unit (amu).
- Protons have a positive charge and a mass of 1 amu.
- Electrons have a negative charge and a mass of 1/1800th the mass of a proton or neutron.
- Neutrons and protons are located in the atomic nucleus.
- Electrons occupy orbitals or shells outside the nucleus.
- The number of protons in an atom is its atomic number.
- Information about elements is shown on the periodic table: including atomic number, symbol, and average atomic mass.
- The number of neutrons can be found by subtracting the atomic number from the atomic mass.
- The number of electrons equals the atomic number of a neutral atom.
- Electron shells can hold specific numbers of electrons: the innermost shell can hold 2; the second can hold 8, etc.
Isotopes
- Isotopes are atoms of the same element that have the same number of protons and electrons but different numbers of neutrons.
- Isotopes have virtually identical chemical properties but different atomic masses.
- Carbon-12, carbon-13, and carbon-14 are examples of carbon isotopes.
Ions
- Ions are atoms or groups of atoms with a positive or negative charge.
- Positive ions are called cations.
- Negative ions are called anions.
- Ions are produced by gaining or losing electrons.
- Ions have important physiological functions in the body.
- Ions are electrolytes.
- Electrolytes conduct an electrical current when dissolved in water.
- Maintaining the balance of electrolytes in the blood is crucial for health.
- Ions can bind together to form ionic compounds (salts).
- Examples of ions include Na⁺, Cl⁻, K⁺, and Ca²⁺
Ionic Bonds
- Ionic bonds are formed by electrostatic interactions between positively charged cations and negatively charged anions.
- These interactions form salts
- The number of positive and negative charges in a salt determine the formula. Examples of ionic compounds include NaCl (table salt), MgCl2, and Ca₃(PO₄)₂.
Covalent Bonds
- Covalent bonds form when atoms share electrons.
- The sharing of electrons results in a molecule.
- Molecules may consist of two or more of the same or different elements.
- The structure of a molecule (how atoms are arranged) can be represented by different formulas.
- Formulas indicate the numbers and types of atoms within a molecule.
- Covalent bonds can be single, double, or triple bonds depending on the number of shared pairs of electrons.
- "octet rule"—atoms tend to gain, lose, or share electrons to attain a complete outer electron shell of 8 electrons. Molecules can be classified as polar or nonpolar, depending on how equally electrons are shared.
- Polar molecules have an uneven distribution of electron density (due to differences in electronegativity), resulting in positive and negative ends. This allows hydrogen bonds to form between water molecules (and between polar molecules), influencing their properties.
- A hydrogen bond is a weak attraction between a hydrogen atom and an electronegative atom in another molecule. This is a type of intermolecular attraction.
- Nonpolar molecules do not have charged ends and generally do not form hydrogen bonds
Intermolecular Attractions
- Intermolecular attractions are weak attractive forces between molecules.
- Hydrogen bonding is a type of intermolecular attraction that occurs between polar molecules.
- Hydrophobic interactions occur between nonpolar molecules in the presence of water.
Water
- Water is essential for life.
- About two-thirds of the human body is composed of water.
- Water has unique properties due to hydrogen bonding.
- Water is a polar molecule, due to unequal sharing of electrons between the oxygen and hydrogen atoms.
- Water's cohesive properties due to hydrogen bonding allow it to stick to itself and other substances (adhesion).
- This makes water a good solvent for many substances.
- Water is a good solvent for polar molecules and ions, forming hydration shells around the dissolved substance.
- When a solute dissolves in water, its individual particles become surrounded by water molecules.
- Water has a high heat capacity, resisting temperature changes.
- Water has a high heat of vaporization
- These properties of water are essential for maintaining homeostasis in living organisms.
Mixtures
- Mixtures are formed when two or more substances are mixed together.
- Mixtures are classified as suspensions, colloids, and solutions based on the size of the particles within the mixture.
- Suspensions are mixtures where particles of one substance are large and will eventually settle out of the mixture.
- Colloids are mixtures where the size of the particles is small enough that they remain suspended but may scatter light.
- Solutions are mixtures where the solute particles are dissolved in the solvent to the point that they are indistinguishable.
Macromolecules
- Macromolecules are large molecules comprised of many smaller molecules (monomers).
- Carbohydrates, lipids, proteins, and nucleic acids are the four major macromolecules in the human body.
- Carbohydrates are the primary source of energy for the body, consisting of monosaccharides, disaccharides, and polysaccharides, such as glycogen.
- Lipids are nonpolar (or partially nonpolar) molecules, such as fats, oils, phospholipids, and steroids.
- Proteins are polymers of amino acids, which have many functions, such as enzymes, structural components, and hormones. The primary amino acid sequence dictates the protein's three-dimensional shape, which determines its function.
- Nucleic acids–DNA molecules carry genetic information and RNA molecules are essential for protein synthesis.
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Description
This quiz covers the fundamental aspects of atomic structure and matter. Explore the classification of matter, the properties of atoms, and the arrangement of elements on the periodic table. Test your knowledge on the composition of atoms and the significance of different elements in the human body.
