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89 Cards in this Set
- Front
- Back
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Matter
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Is anything that takes up space and has a mass.
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Mass
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Is the quantity of matter an object has
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Elements
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Substances that can not be broken into similar types of matter
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What is the smallest part of an element
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An atom
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Protons
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Are positively charged found in the nucleus of an atom
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Atomic number
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The number of protons in the nucleus
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Neutrons
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Are neutral subatomic particles found in the nucleus of an atom
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Electrons
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Negatively charged atoms in various energy levels (orbital shells)
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Chemical reaction
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A dynamic event that alters the chemical make up of an atom , may cause an imbalance in the charge, resulting in excess protons or electrons
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Ion
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When an imbalance produces positively or negatively charged atom
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What does a proton and neutron have in common
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Same mass
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Mass number
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Is the total number of protons and neutrons found within the nucleus of an atom
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Atomic mass
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Is the average mass of all known isotopes of an element.
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How do you get the neutron number
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By taking the mass number and subtracting it by the atomic number
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Charge
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Refers to the positive or negative distribution in an atom
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What is a charge dominated by
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The number of protons and electrons
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Isotopes
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Atoms with the same number of protons, but different number in neutrons
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Catalysts
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Control the rate of chemical reactions or reactions in which atoms come to a stable state
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What the reaction rates depend on
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The fluency of contact with the reactants and catalysts
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Substrate
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Molecular surface acted upon by an enzyme
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Activation energy
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Catalysts increase reaction rates by lowering this... The potential barrier of products compared to reactants is reduced, resulting in a reaction path requiring less energy
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The Four step process of a general reaction
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1.) X + C---> XC
2.) XC + Y-->XYC 3.)XYC--> CZ 4.)CZ-->C +Z |
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Orbital shells
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The arrangement of electrons within orbits around the nucleus
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Valence electrons
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Electrons in the outermost shell of an atom remain the same
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Electro negativity
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Measure of an atoms attraction on electrons in a chemical bond
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Chemical bonding
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The chemical merging of atoms due to their electron arrangements
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Metals
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Elements that donate highly conductive electrons to their environment
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Enzymes
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Act as the catalysts for special chemical reactions within the human body, found in protein molecules
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Globular proteins
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Proteins that are water soluble, built from amino acids that form chains
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External factors that controls cell process activity of enzymes
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Temperature, ph, and substrate concentration
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PH
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Value is a measure of hydrogen ion concentration within a solution, and a substrate is a molecular surface acted upon by an enzyme,
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Metabolic pathways
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Chemical reactions within a cell
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Enzymes can...
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Act to lower the activation energy of chemical reactions, can reshape itself when placed in contact with a substrate, and the amino acid structure of an enzyme is important
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Ph scale
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Measures the strength of acidic solutions (solutions with a ph less than 7) and basic solutions (greater than 7). Water is neutral with a ph of 7
-stronger acids will have smaller value, and stronger bases will have a greater value |
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Ph indicator
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Used to qualitatively determine the ph
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Ionic
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The electrical attraction between ions of opposite charge
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Covalent
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Sharing of electrons between atoms
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Hydrocarbons are...
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Methane, propane, and butane bond to hydrogen to carbon atoms
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Hydrocarbons subdivided into
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Saturated and unsaturated categories
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Alkanes: saturated hydrocarbons
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Basic structure, composed entirely of single bonds and are saturated, with hydrogen.
Formula: is CnH2n+2t |
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Saturated
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Carbon is completely connected
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Unsaturated hydrocarbons
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Have one or more double or triple bonds between carbon atoms, they permit the attachment of other atoms to the unbonded carbon atoms within the molecule
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Alkenes
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Unsaturated hydrocarbons with double bonds, CnH2n
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Alkynes
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Unsaturated hydrocarbons that contain triple bonds, CnH2n-3
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Organic chemistry
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Connected with the study of hydrocarbon structure
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Metalloids
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Are elements that may accept or donate electrons readily, and possess a mixture of metallic and nonmetallic properties
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Cation (metallic ion)
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Positive ion
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Anion(nonmetallic)
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A negative ion
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Ionic bonds
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Complete one another by the donation and acceptance of electrons to form stable outer electron shells. Ex. Table salt
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Covalent bonds
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Is a form of chemical bonding that involves electron sharing between atoms, valence electrons are being shared to form a stable outer shell for both atoms. Greatest between atoms of similar electro negativity
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Electro negatives
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Similar attractions for electrons
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Lewis Structures
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Provide visual representations of covalent bonding between atoms or a molecule. The atoms are symbolically shown and surrounded by dots that represent each of the valence electrons. The dots are arranged such that molecules is shown to have atoms in the most completely filled shell configuration of paired electrons
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Balancing chemical equations
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Reactions must be balanced according to atomic number and charge. The goal is to make sure that their are equal numbers of each atom on the reactant side and the product side
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Reactants
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Formulas on the left side of the reaction side, are substances that have been consumed or altered
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Products
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Are located on the right side of the reaction side, there are the substances formed
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Subscripts
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Formulas where equations have small numbers, they indicate how many atoms of an element are in the formula
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Oxidation reduction and acid base reactions
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Involve the donation and acceptance of electrons
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Oxidation
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Involves electron domination to produce a more positive ion
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Reduction
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Involves electron acceptance to produce a more negative ion
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Oxidation reduction reactions
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Combustion, photosynthesis, metabolism
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Metabolism
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Refers to the chemical reaction in living organisms that area nessacary to maintain life
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Light years
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The distance that light traveled within one year of time
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Electromagnetic waves
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Are waves of radiation that are characterized by electric and magnetic fields
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Work
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The results of any change in energy
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Joules or calories
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Work is quantified in units of the metric system
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(KE) kinetic energy
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Energy of motion, any increase in an objects velocity
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(PE) potential energy
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The amount of stored energy in an object may be quantified through a calculation
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Law of conservation of energy
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Energy is not lost but rather transferred back and fourth between KE and PE, given an amount of total energy in the system, and increase in KE will result in a decrease in PE (vice versa) but the total amount of energy will remain the same
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Water
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A polar molecule of hydrogen and oxygen with oxygen possessing the higher electronegativeity
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Polar molecule
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A molecule that possess both positive and negative atomic structure
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Electrolysis
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Can chemically split the liquid water molecule into gaseous components according to the balanced equation 2H2O-->2H2+O2
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Density
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Is the ratio of mass per volume for a substance, water is 4 C
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Celsius
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Is a metric temperature scale that is defined by standard pressure by the melting point of ice 0 and the boiling point of water 100c
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Kelvin Scale
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Used to express temperature , scaled defined by the absolute zero reference point
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Triple-point
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The temperature of which water will coexist as a solid liquid or gas
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Specific heat
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The energy required to raise one unit of mass by substance by 1 C
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High heat evaporation
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E amount of heat nessacary to cause a phase transition between a liquid and a gas
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Water
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Polarity results in high surface tension and adhesion. Essential to metabolic process
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Anabolic
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Creation of larger molecules
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Catabolic
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Creation of smaller molecules
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Temperature
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Directly related to the speed of particles and pressure is the force of particle interaction over a certain area
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Solid
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Has a fixed shape and volume, possesses crystalline order, relatively high pressures and low temperatures
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Crystalline order
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Atoms are arranged in highly ordered state, a state in which atoms lack true order
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Physical bonding
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Physical connection between atoms or molecules, that does not alter the chemical nature of atoms
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Gas
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Changing volume and changing shape
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Latent heat
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Related to the energy needed to cause a phase transition at a fixed temperature
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Heat
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The flow of energy due to a difference in temperature
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Evaporation
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Of a liquid is often achieved due to high heat, low humidity, and fast movement surrounding air mass. It occurs by physical collisions at the surface layer of a liquid, removes the fast moving liquid molecules,there by removing nome energetic atoms from the liquid
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Vaporization: phase transition
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Is an alteration of a physical state between a solid, liquid and gas. This transition from a liquid to a gas takes place by breaking the physical bonds with in the liquid
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