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| All living things are composed of ______. |
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Definition
| anything that occupies space and has mass |
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| Matter exits in what 3 states? |
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| force of gravity acting on mass |
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| What does the Law of Conservation of Energy state? |
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Definition
| Energy cannot be created nor destroyed; instead it remains constant |
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| What are 2 types of energy? |
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Definition
| Kinetic Energy and Potential Energy |
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Definition
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| inactive or stored energy |
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Definition
| Radiant, Heat, Mechanical, Electrical, Chemical |
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Definition
| energy that travels in waves (micro, light, UV, x-rays) |
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| What is Electrical Energy? |
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Definition
| energy resulting from the flow of charged particles (electricity powering computer/heart) |
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Definition
| energy transferred from one object to another due to difference in temperature (cooling) |
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Definition
| energy released or used in the process of destroying or forming chemicals |
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| What is Mechanical Energy? |
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Definition
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| When is Mechanical Energy Potential / Kinetic? |
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Definition
| Potential: object is still. Kinetic: object is moving |
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Term
| What are the building blocks of all forms of matter? |
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Definition
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Term
| How many elements exist? How many are naturally occurring? How many occur in the human body? |
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Definition
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| What elements make up 96% of human body mass? |
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Definition
| CHON: Carbon, Hydrogen, Oxygen, Nitrogen |
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Term
| The smallest unit of matter? |
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Definition
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Term
| Fill in the blank: A(n) ___(A)___ is a quantity of ____(B)____ composed of ___(C)___ of the same type. |
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Definition
| A: Element; B: Matter; C:Atoms |
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Term
| An atom is made up of what? |
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Definition
| Subatomic particles called protons, neutrons, and electrons |
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Definition
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Term
| Which has a positive charge? |
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Definition
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| Which has a negative charge? |
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Definition
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Term
| How many electrons can each of the 3 Electron shells hold? |
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Definition
1st: 2;
2nd: 8;
3rd: max 18 |
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Term
| The atomic number is based on what? |
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Definition
| number of protons in the nucleus |
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| The mass number is based on what? |
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Definition
| number of protons and neutrons in the nucleus |
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Term
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Definition
| an atom of an element with the same amount of protons, but different amount of neutrons |
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Term
| What happens to an unstable isotope? |
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Definition
| as they lose stability, they decay into more stable forms causing them to emit radioactivity (packets of energy) |
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Definition
| the total mass of an atom's protons, neutrons, and electrons when at rest |
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Definition
| charged particles in which there is no longer an equal number of protons and neutrons |
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Term
| What process forms Ions and how? |
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Definition
| Ionization; forms when an atom either gives up or receives an electron |
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Term
| Next to a chemical symbol, what does the ( + ) and ( - ) mean? |
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Definition
( + ) ---> this chemical gave up an electron
( - ) ---> this chemical received an electron |
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Definition
| an atom negatively charged from gaining an electron |
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Definition
| an atom positively charged from losing an electron |
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Term
| How does a molecule form? |
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Definition
| 2 or more atoms come together in a chemical reaction by sharing or exchanging valence electrons |
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Term
| When forming a molecule, can the atoms be the same or do they have to be different? |
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Definition
| They can be the same or different |
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Definition
| a chemical substance composed of 2 or more different elements by a chemical reaction |
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Definition
| an electrically charged atom or groups of atoms with an unpaired electron in its outermost shell (valence) |
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Term
Is a Free Radical stable?
Why?
How does it become stable? |
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Definition
No
It has an unpaired electron.
By giving up the unpaired electron or taking an electron from another molecule. |
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Term
| Studies suggest that you can take what to prevent Free Radical induced damage? |
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Definition
| Antioxidants- they lack an electron, which causes them to bind with the Free Radicals |
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Term
| What are the products of a chemical bond? |
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Definition
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Definition
| The explanation why atoms interact in a chemical reaction; Ideally, every atom (except H and He) want 8 electrons in their valence shell |
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Term
| What are the 3 types of chemical bonds? |
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Definition
| Ionic bond, Covalent bond, Hydrogen bond |
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Term
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Definition
| Ions are joined and one or more electrons are TRANSFERRED between atoms |
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Definition
| Forms when two atoms SHARE one or more pairs of electrons |
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Term
| What makes a covalent bond stronger? |
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Definition
| More pairs of electrons shared |
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Term
| Can Ionic bonds form between two atoms of the same element? |
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Definition
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Term
| What is a polar covalent bond? |
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Definition
| when shared electrons orbit one nucleus more than the other |
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Term
| What is a non polar covalent bond? |
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Definition
| when shared electrons orbit each nucleus equally |
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Term
| Hydrogen bonds confer _____, _______, and ______. |
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Definition
| Strength, Stability, and Shape |
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Term
| When do chemical reactions occur? |
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Definition
| When new bonds form or old bonds break |
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Term
| What is an exergonic reaction? |
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Definition
| when the amount of energy RELEASED is MORE than energy ABSORBED |
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Term
| What is an energonic reaction? |
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Definition
| when the amount of energy ABSORBED is MORE than what can be RELEASED |
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Term
| What is Activation Energy? |
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Definition
| Kinetic; the amount of energy needed to disrupt the electronic stability of a molecule; energy needed to start reactions |
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Term
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Definition
| a reusable substance that speeds up chemical reactions by lowering the activation energy |
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Term
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Definition
| a substance that dissociates into one or more hydrogen ions (H+) and one or more ions |
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Definition
| a substance that dissociates into one or more hydroxide ions (OH-) and one or more ions |
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Definition
| a substance that dissociates into cations and anions, NEITHER of which are OH- or H+ |
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Definition
| Universal solvent, thermal stability, cohesion, chemical reactivity |
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