Test #1
Inquiry~ Search for information and explanations
Scientific process~Observation, Question, Hypothesis, Prediction, and experiment
Prediction: statement
Qualitative~Recorded data
Quantitative~ Numerical data (numbers only)
Inductive reasoning - logical process of induction: Large number of specific observations
Hypothesis – testable and falsifiable: No hypothesis can be proven true, only supported, but can be proven false
Experiment~ Scientific test carried out under controlled conditions
Deductive reasoning~ to make specific predictions
controlled experiment~ You can change ONE thing at a time
independent variable~ What changes or changing
Dependent variable~ What’s being affected by the change
Theory~ Only supported by numerous studies
Matter~ Takes up space and has mass (Made of elements, Chemical/physical property and cannot be broken down into substances)
Element~ Cannot be broken down further by chemical reactants (Pure substance that occurs naturally in)
Compound~ Has two or more elements
Essential elements – 92
Carbon, hydrogen, oxygen, and nitrogen – 96%
Calcium, phosphorus, potassium, and sulfur – 4%
Trace elements~ required for life in minute quantities
Atom~ Smallest unit of matter that still retains the properties of an element
Neutrons (no electrical charge) ( are found in the nucleus of an atom and contribute to the atomic mass along with protons)
Protons (positive charge) (+)
Electrons (negative charge) (-)
Atomic number~ # of protons
Mass number~ # of protons AND neutrons in an atom
Atomic mass~ element’s total mass across all atoms in existence
Isotopes ≠ number of neutrons (Two atoms, same element, differ in # or neutrons)
Radioactive isotopes~ Decay spontaneously living off particles and energy
Chemical Properties~ are characteristics of a substance that become apparent during a chemical reaction and describe how a substance behaves in the presence of other substances (Reactivity, Flammability, corrosiveness, and stability)
Valence shell~ the outer shell of the atom
Octet rule~ Describes an atom’s preference for having 8 electrons in its valence shell
Chemical bonds~ Hold molecules together and create temporary interactions between atoms, allowing them to form stable compounds or participate in chemical reactions.
Covalent bonds: Involves the sharing of electrons
The different covalent bonds are: Single bond, double bond, and triple bond
Electronegativity – The force of attraction between atom and electrons it’s sharing in a covalent bond with another atom
Polar bonds~ One atom is electronegative, and do NOT share electron equally
Nonpolar bonds~ The atoms share the electron equally
Ionic bonds (When anions and cations attract each other): anion - and cation +
Hydrogen bonds~ Hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom
Van der waals~ Attraction between 2 molecules due to accumulation of electrons in certain regions
Molecular Mass: sum of all masses of all atoms in a molecule
Binding to endorphin receptors
Chemical reactions are reactants, products, and chemical equilibrium
Reactants~ Used to make products (Ingredients)
Products~ Final thing made
Chemical equilibrium~ Reached when forward and reverse reactions occur at the same rate
Water - polar molecule
Covalent bonds: Formed when atoms share electrons, resulting in a stable balance between the attractive and repulsive forces between atoms.
Three types of Covalent bonds: Single, double, and triple
Cohesive keeps water molecules together
Adhesion keeps water molecules from failing downward
Heat:Thermal energy transfer from one body of matter to another
Temperature: average kinetic energy of molecules
Expansion upon freezing: Hydrogen bonds expand, making it ice denser than water
Solvent~ dissolving agent (Liquid)
Solute~substance being dissolved (Salt)
Solution~liquid that is completely homogeneous mixtures of substances
hydrophilic~ substance that is attracted to water
hydrophobic~ substance that is NOT attracted to water
Acid~ Increase H+
Bases~ Decreases H+
Buffers~ substances that minimize changes in pH
H+: Hydrogen Ion
OH-: Hydroxide Ion
Living organisms – carbon based
Carbon – explain the versatility CHONPS
Organic compounds – small or colossal molecules
Organic chemistry~ study of compounds containing carbon
C, H, O, N, S, and P—are quite uniform from one organism to another
Macronutrients:
Carbohydrates: Provide energy, made up of sugars and starches.
Proteins: Essential for growth, repair, and enzymatic functions; composed of amino acids.
Fats: Important energy source, involved in cell membrane formation, storage, and absorption of fat-soluble vitamins.
trace elements~ Chemical element of a minute quality
Carbon form 4 bonds
Carbon chains vary in length and shape
Hydrocarbons - only carbon and hydrogen
Isomers~Compound w/ same molecular formula but different structures
Structural isomers~ different covalent bonds and arrangement of atoms
Cis-trans isomers~ same bonds but different spatial arrangements
Enantiomers~ mirror images of each other
ATP~ main energy source for cells
Kinetic energy~ energy of motion
Thermal energy~ energy due to random molecular motion
Orbital- 3D space around which electrons orbit (2 electrons PER orbital)
Electron shells- fixed areas in which electrons can orbit at set distances from the nucleus