Term
| All forms of matter are composed of one or more elements. Be able to list the major elements in living things. |
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Definition
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Term
| Define the terms atomic number and atomic mass and be able to describe their significance. |
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Definition
| Atomic number is the number of protons an atom has. It’s unique for each element. Atomic mass is the number of protons and neutrons in an atom. The number can change for elements that are isotopes. |
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Term
| Atoms with the same atomic number but a different mass number are isotopes. List the isotopes of hydrogen and of carbon. |
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Definition
| Hydrogen, Deuterium, Tritium Carbon-12, Carbon-14 |
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Term
| Be able to describe radioisotopes and list three ways they are used in biology. |
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Definition
| Radioisotopes are isotopes that spontaneously decay, releasing radioactivity. They can determine the diet of ancient peoples, age of fossils and artifacts, and they’re the source of radiation used in medical diagnostic and treatment procedures. |
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Term
| The union between the electron structures of atoms is known as the chemical bond. Be able to list and describe the three types of chemical bonds found in living things. |
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Definition
| Ionic bond: atoms that don’t have a full outermost orbital either lose or gain electrons from other elements in order to be “happy”. And, once they’re “happy” an atom gets a charge. Opposite ions attract. Covalent bond: when atoms share electrons. There can be single, double, and triple bonds. When electrons spend more time with 1 atom in the covalent bond than with another, so a polar covalent bond forms. |
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Term
| Be able to describe the distribution of electrons in the space around the nucleus of an atom. |
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Definition
| Starting from the inner orbital: 2, 8, 18, 32 |
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Term
| An atom tends to react with other atoms when its outermost shell is only partly filled with electrons. Be able to discuss why this happens. |
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Definition
| It’s kind of an atom’s goal to have a full outermost shell. So an atom will either lose, gain, or share electrons with another atom. |
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Term
| Be able to define the two types of ions and describe how ionic bonds form between positive and negative ions. |
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Definition
| Cation (+) and Anion (-) Normally atoms are neutral, but to gain stability they’ll lose 1 or more of their outer electrons and become + or gain 1 or more electron and be -. Once this happens opposites will attract, forming an ionic bond. |
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Term
| In a covalent bond, atoms share electrons. List several elements that tend to form covalent bonds. |
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Definition
| Hydrogen and carbon, oxygen, nitrogen, hydrogen and oxygen |
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Term
| Distinguish between a nonpolar covalent bond and a polar covalent bond and give an example of each. |
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Definition
| A polar covalent bond is when the electrons that are being shared spend more time with 1 atom than the other. Ex: water A nonpolar is a normal covalent bond. Ex: Oxygen gas |
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Term
| Define hydrogen bond and describe conditions under which hydrogen bonds form and cite one example. |
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Definition
| A weak bond between 2 atoms (1 is hydrogen) with partially opposite charges. Ex: ice and in amino acids |
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Term
| Explain what is meant by the polarity of the water molecule, and how the polarity of water molecules allows them to interact with one another. |
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Definition
| Because the oxygen in water has a greater electronaffinity the electrons spend more time with it resulting in apolar covalent bond. So, the oxygen end of the molecule is - and hydrogen is slightly +. The water is polar because it has 2 charges. The polarity of water causes it to be attracted to other polar molecules, which is why water can interact with water. |
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Term
| The outermost electron shell of every Noble Gas element (except Helium) has ___ electrons. |
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Definition
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Term
| The chemical bond between water molecules is a ___ bond. |
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Definition
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Term
| A solution with a pH of 7 has ___x more H ions than a solutrion of pH 9. |
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Definition
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Term
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Definition
| Units of two or more atoms held together by chemical bonds. The combination of atoms by chemical bonds with the component atoms in definite porportions, such as water (two H to one O). |
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