Chemistry Basics Quiz

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.