Term
| What is all matter composed of? |
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Definition
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Term
| What are 2 characteristics of matter? |
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Definition
1.) Has mass
2.) Occupies space |
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Term
| What are the 3 components of atoms? |
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Definition
1.) Protons
2.) Neutrons
3.) Electrons |
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Term
| What are the relative masses of protons, neutrons, and electrons? |
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Definition
| Protons and neutrons have roughly the same mass where electrons have a much smaller mass |
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Term
| What makes up an atomic number? |
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Definition
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Term
| Atoms with the same atomic number have the same chemical properties and belong to the same ___________. |
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Definition
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Term
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Definition
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Term
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Definition
| The force of gravity exerted on something. It is mass in the concept of gravity. |
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Term
| What makes up atomic mass? |
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Definition
| The sum of protons and neutrons |
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Term
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Definition
| Same # of protons, different number of neutrons. |
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Term
| Radioactive isotopes are what? |
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Definition
| Unstable and emit radiation as the nucleus breaks up. |
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Term
| What do we use radioactive isotopes for? |
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Definition
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Term
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Definition
| The time it takes for one-half of the atoms in a sample to decay. |
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Term
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Definition
| Negatively charged particles with very small mass |
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Term
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Definition
| Same # of protons and electrons |
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Term
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Definition
| A charged atom. Different number of protons and electrons |
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Term
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Definition
| Fewer electrons than protons. Positively charged. |
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Term
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Definition
| Have more electrons than protons. Negatively charged. |
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Term
| Are cations usualy oxidized of reduced? |
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Definition
| Oxidized, easier to lose than to gain. |
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Term
| Are anions usually oxidized or reduced? |
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Definition
| Reduced, easier to gain than to lose. |
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Term
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Definition
| where we can predict the location of an electron |
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Term
| What does electron arrangement effect? |
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Definition
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Term
| How many electrons can each orbital contain? |
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Definition
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Term
| What do electrons posses? How does their location effect this? |
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Definition
| Potential energy. Further from nucleus, more energy. |
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Term
| Energy LEVELS are different from energy ORBITALS how? |
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Definition
Levels = energy
Orbital = location |
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Term
| Electrons can be transferred from one atom to another while retaining what? |
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Definition
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Term
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Definition
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Term
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Definition
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Term
| How do periodic tables display elements? |
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Definition
| According to valence electrons |
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Term
| What is a valence electron? |
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Definition
| Number of electrons in outermost energy level. |
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Term
| Non reactive elements have how many valence electrons? |
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Definition
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Term
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Definition
| Completely full outer energy levels. (8) |
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Term
| How many naturally occurring elements are there? |
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Definition
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Term
| How many elements are found in living organisms? |
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Definition
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Term
| What 4 elements make up 96.3% of human body weight? |
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Definition
| Carbon, Hydrogen, Oxygen, and Nitrogen |
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Term
| What make up organic molecules? |
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Definition
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Term
| Atoms with full energy levels are less or more reactive than those with unfilled energy levels? |
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Definition
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Term
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Definition
| Groups of atoms held together in a stable association. |
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Term
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Definition
| Molecules containing more than one type of element |
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Term
| What are atoms held together by? |
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Definition
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Term
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Definition
| Electrostatic interations between 2 molecules that can be disrupted by electrical attraction with water molecules. |
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Term
| Which is stronger: ionic or covalent? |
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Definition
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Term
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Definition
| Form when atoms share 2 of more PAIRS of valence electrons. |
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Term
| Is there a charge with covalent bonds? |
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Definition
| No, no net charge, satifies octet, no unpaired electrons. |
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Term
| What is the strength of a covalent bond dependent on? |
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Definition
| The number of shared electrons. |
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Term
| What do chemical reactions involve? |
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Definition
| The formation or breaking of chemical bonds. |
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Term
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Definition
| The original molecule in a reaction |
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Term
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Definition
| Molecules resulting from a reaction. |
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Term
| 6 H20 + 6 CO2 -> C6H12O6 + 6 O2 is what? |
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Definition
| Photosynthesis. The product is glucose. |
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Term
| What influences chemical reactions? |
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Definition
1. Temperature
2. Concentration of reactants to products
3. Catalysts |
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Term
| Electronegativity is an atom's what? |
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Definition
| Affinity for electrons. How greedy an atom is for electrons in the structure of a covalent bond. |
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Term
| What does differences in EN dictate? |
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Definition
| How electrons are distributed in a covalent bond |
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Term
| Nonpolar covalent bonds have unequal or equal sharing of electrons? |
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Definition
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Term
| Polar covalent bonds have unequal or equal sharing of electrons? |
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Definition
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Term
| In a nonpolar covalent bond, where are the electrons located? |
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Definition
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Term
| In a polar covalent bond, where are electrons located? |
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Definition
| They are closer to the element with the higher EN |
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Term
| What is the EN level for Oxygen? |
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Definition
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Term
| What is the EN level for Nitrogen? |
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Definition
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Term
| What is the EN level for Carbon? |
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Definition
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Term
| What is the En level for Hydrogen? |
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Definition
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Term
| What is an important characteristic of water? |
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Definition
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Term
| Which bonds in H2O are highly polar? |
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Definition
| the bonds between hydrogen and oxygen |
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Term
| Oxygen is partially _______ while hydrogen is partially ________. |
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Definition
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Term
| Are water molecules polar or nonpolar? |
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Definition
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Term
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Definition
| A weak attraction between the partially negative oxygen of one water molecule and the partially positive hydrogen molecule of a DIFFERENT water molecule. |
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Term
| What can hydrogen bonds form between? |
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Definition
1.) Between water molecules
2.) Between water and another charged molecule |
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Term
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Definition
| Water molecules sticking to each other by hydrogen bonds. Causes surface tension. Only occurs with other water molecules. |
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Term
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Definition
| Water molecules sticking to other polar molecules by hydrogen bonding. Can be water, can be just another polar molecule. |
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Term
| What are 6 properties of water? |
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Definition
1.) Has high specific heat which requires a large amount of energy. This is so other organisms do not boil.
2.) Water has a high heat of vaporizing. The evaporating of water form a surface causes cooling of a surface. Sweating.
3.) Solid water is less dense than liquid water. Ice floating in drinks
4.) Water is a good solvent because is dissolves polar molecules and ions. Universal solvent.
5.) Water organizes nonpolar molecules. Hydrophilic = water loving. Hydrophobic = water fearing. Water causes hydrophobic molecules to assume specific shapes.
6.) Water can form/break apart into ions.
H2O -> OH- + H+ |
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Term
| What do water molecules aggregate around? |
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Definition
| It's respective charge. Postive aggregates around negative and vice versa. |
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Term
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Definition
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Term
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Definition
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Term
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Definition
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Term
| pH is the negative logarithm what? |
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Definition
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Term
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Definition
| Any substance that disassociates in water to increase the H+ concentration/lowers pH |
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Term
| The stronger the acid, the more _______ it produces |
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Definition
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Term
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Definition
| A substance that combines with H+ in water and lowers the H+ concentration. |
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Term
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Definition
| Any substance that resists changes in pH |
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Term
| How does a buffer act when a base is added? |
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Definition
| Releases H+ ions, raising the pH |
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Term
| How does a buffer act when an acid is added? |
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Definition
| Absorbing H+ ions, lowers the pH |
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Term
| What does the range of effectiveness depend on? |
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Definition
| Particular types of buffers |
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Term
| What do most biological buffers consist of? |
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Definition
| A pair of molecules; one acid and one base. |
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