Term
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Definition
| The sum of all the chemical reactions that occur in your body. |
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Term
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Definition
| Anything that occupies space and has mass. |
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Term
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Definition
| Substance that cannot be broken down by chemical reactions |
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Term
| How many naturally occurring elements are there? |
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Definition
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Term
| True or False. Everything is made up of matter. |
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Definition
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Term
| How many elements are essential to people? |
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Definition
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Term
| How many elements do plants need? |
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Definition
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Term
| Periodic Table of Elements |
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Definition
| A table of all of the chemical elements, naturally occurring and synthetic. |
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Term
| How are the elements ordered in the periodic table? |
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Definition
| Elements are ordered by their atomic number. |
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Term
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Definition
| Number of protons in the nucleus of an atom. |
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Term
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Definition
| The average mass of an atom of that element. |
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Term
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Definition
| Elements that are required in very small amounts, but they are essential for life. |
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Term
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Definition
| Substances that contain 2 or more elements in a fixed ratio. |
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Term
| When elements combine, what do they form? |
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Definition
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Term
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Definition
| The amount of material in an object. |
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Term
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Definition
| basic building block of all matter. |
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Term
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Definition
| Particles that create an atom, such as electrons, neutrons, and protons |
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Term
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Definition
| Positively charged subatomic particle |
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Term
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Definition
| Negatively charged subatomic particle |
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Term
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Definition
| Neutrally charged subatomic particle |
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Term
| What happens when an atom has an equal number of protons and electrons? |
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Definition
| The atom's electrical charge is zero and the atom is neutral. |
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Term
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Definition
| Location of the neutrons and protons in an atom. |
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Term
| Where are electrons located? |
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Definition
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Term
| How many naturally occurring elements are used by a person's body? |
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Definition
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Term
| Which elements are the most abundant in living cells? |
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Definition
| Oxygen, carbon, hydrogen, and nitrogen |
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Term
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Definition
| forms of an element that differ in mass. |
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Term
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Definition
| Isotope in which the nucleus decays spontaneously, shedding particles and energy. |
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Term
| What is a consequence from exposure to a radioactive isotope? |
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Definition
| Radiation from decaying isotopes can damage cellular molecules and thus pose serious health risks. |
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Term
| By definition, all atoms of carbon have how many protons in their nucleus? |
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Definition
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Term
| What changes between an element and its isotope? |
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Definition
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Term
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Definition
| An attractions between two atoms resulting from a sharing of outer-shell electrons or the presence of opposite charges on the atoms. |
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Term
| What are the three types of chemical bonds? |
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Definition
| Ionic, covalent, and hydrogen bonds. |
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Term
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Definition
| atoms that are electrically charged as a result of gaining or losing electrons. |
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Term
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Definition
| Bond formed between oppositely charged ions. |
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Term
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Definition
| Compounds held together by ionic bonds. |
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Term
| The suffix -ide is used when? |
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Definition
| It is used for ionic compounds. |
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Term
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Definition
| An attraction between atoms that share one or more pairs of electrons. |
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Term
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Definition
| Elements (2 or more atoms) that are held together through a covalent bond. |
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Term
| Which type of bond is the strongest? |
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Definition
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Term
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Definition
| A weak chemical bond formed when a partially charged hydrogen atom from one polar molecule is attracted to a partially negative atom in another molecule. |
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Term
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Definition
| A molecule containing an uneven distribution of charge due to the presence of polar covalent bonds. |
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Term
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Definition
| Process leading to chemical changes in matter, involving the making and breaking of chemical bonds. |
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Term
| Are atoms destroyed in chemical reactions? |
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Definition
| No, they are only rearranged. |
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Term
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Definition
| Starting material in a chemical reaction. |
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Term
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Definition
| Ending materials in a chemical reaction. |
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Term
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Definition
| Cohesiveness, Temperature moderation, Density, Solvent |
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Term
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Definition
| Water molecules attraction to self because of hydrogen bonds. |
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Term
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Definition
| Measure of how difficult it is to stretch or break the surface of a liquid. |
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Term
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Definition
| Property of water whereby a body becomes cooler as water evaporates from the surface. |
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Term
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Definition
| Ice floats because it's less dense than the water its floating in. |
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Term
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Definition
| Ice floats because of surface tension due to the cohesion of the water molecules and because it's less dense than liquid water. |
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Term
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Definition
| A liquid consisting of a homogeneous mixture of 2 or more substances. |
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