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Biology #2

TermDefinition
Importance of Chemistry in Biology Chemistry provides the founda9on for understanding how biological molecules interact and function.
Matter Anything that has mass and occupies a space
Mass Amount of matter a substance contains
Element A substance that cannot be broken down into substances with different properties (one type of atom)
Basic Atomic Structure Atoms, Subatomic Particles (Protons, Neutrons, Electrons) Atomic Number, Atomic Mass, Isotopes
Atoms The smallest unit of matter that retains the proper9es of an element
Protons Positively charged particles in the nucleus
Neutons Neutrally charges particles in the nucleus
Electrons Negatively charged particles orbiting the nucleus
Atomic Number The number of protons in an atom’s nucleus, which defines the element
Mass Number The sum of protons and neutrons in the nucleus.
Isotopes Atoms of the same element with different numbers of neutrons.
CHNOPS The 6 elements that make up 95% of the bodyweight of organisms. Carbon, Hydrogen, Nitrogen, Oxygen, Phosphorus, Sulfur
Periods Atoms arranged horizontally in the periodic table
Groups Atoms arranged vertically in the periodic table
Valence Shell Determines many of an atom's chemical property
Octet Rule Outermost shell is most stable when it has EIGHT electrons in the outer shell
Molecule Two or more of the same type of atom bonded together
Compound Molecule containing at least two different elements bonded together
Formula Number of each kind of atom in a molecule
Examples of Compound Elements C O2, H2 O, C6 H12 O6
Ion Atom that's gained or lost an electron
Elements (in simple terms) Pure substances consisting of only one type of atom
Chemical Bonds Ionic Bonds, Covalent Bonds, Hydrogen Bonds ; Nonpopular Covalent Bonds, Polar Covalent Bonds
Ionic Bonds Formed when electrons are transferred from one atom to another, creating ions (Sodium chloride NaCl)
Covalent Bonds Formed when atoms share one or more pairs of electrons (Water- H2O)
Hydrogen Bonds Weak bonds that form between a hydrogen atom covalently bonded to an electronegative atom and another electronegative atom
Nonpolar Bonds Electrons are shared equally between atoms
Polar Covalent Bonds Electrons shared unequally
Electronegativity Ability of an atom to attract electrons toward itself in a chemical bond
Reactants and Products Reactants are the starting materials in a reaction; products are the substances formed as a result of the reaction
Solution Contains dissolved substances or Solutes
Properties of Water Polarity, Cohesion, Adhesion, High Specific Heat, Universal Solvent
Polarity Water is a polar molecule, meaning it has a partial positive charge on one end and a partial negative charge on the other
Cohesion Water molecules stick to each other due to hydrogen bonding
Adhesion Water molecules stick to other surfaces
High Specific Heat Water can absorb a lot of heat without a significant change in temperature
Universal Solvent Water can dissolve many substances due to its polarity
pH A measure of hydrogen ion concentration in a solution
pH Scale Measures the concentra9on of hydrogen ions (H⁺) in a solution. Ranges from 0 (acidic) to 14 (basic), with 7 being neutral.
Acids Substances that donate H⁺ ions (e.g., hydrochloric acid, HCl)
Bases Substances that accept H⁺ ions or donate OH⁻ ions (e.g., sodium hydroxide, NaOH)
Buffers Substances that help maintain a stable pH by neutralizing excess acids or bases.
Created by: kassa.cool
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