Term
| What is the Quantum leap or atomic spectra process? |
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Definition
| electrons absorb energy and jump up to the excited state -- the release energy as light (colors) and jump down to a lower level |
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Term
| How are metals and nonmetals different? |
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Definition
| metals are good conductors and are usually silver/grey and malleable, but nonmetals are poor conductors and are brittle |
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Term
| What are valence electrons? |
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Definition
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Term
| When are elements SIMILAR? |
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Definition
| If they are in the same group/ same valence electrons |
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Term
| What is the atomic number? |
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Definition
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Term
| What is the number of neutrons? |
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Definition
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Term
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Definition
| same element, same atomic number, different mass, different neutrons |
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Term
| What is the atomic mass (average)? |
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Definition
| Average of an isotope's masses |
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Term
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Definition
| a high probability area outside the nucleus where electrons are located |
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Term
| Where are electrons located? |
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Definition
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Term
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Definition
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Term
| What are the numbers of protons and electrons in a neutral atom? |
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Definition
| protons and electrons are the same number in a neutral atom |
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Term
| When an atom loses electrons, what happens to the mass? |
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Definition
| nothing - electrons weigh almost 0 amu |
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Term
| What is the mass of a proton or neutron? |
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Definition
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Term
| What is Ionization Energy? |
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Definition
| the amount of energy it takes to remove an electron |
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Term
| How does Ionization energy change as you go across a period? Why? |
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Definition
| IE increases as you go across the table because atoms get smaller and hold onto their electrons more tightly. so it takes more energy to remove them |
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Term
| How does Ionization energy change as you go down a group? Why? |
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Definition
| IE decreases as you go down the table because atoms get larger and hold onto electrons more loosely, so it takes less energy to remove them |
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Term
| How does Atomic Radius change as you go across a period? |
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Definition
| Radius gets smaller as you go across because the nucleus pulls the electrons into more closely and more tightly |
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Term
| How does Atomic Radius change as you go down a period? |
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Definition
| Radius gets larger as you go down a group because there are more shells and the electrons are held more loosely |
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Term
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Definition
| Draw the nucleus and write the protons and neutrons inside. Then draw the shells/rings and use the electron configuration from the periodic table to put the electrons in the shells. |
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Term
| How do you draw a LEWIS diagram? |
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Definition
| Write the symbol and put the dots to represent the VALENCE (outer) electrons only |
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Term
| What is electronegativity? |
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Definition
| The ability to attract electrons |
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Term
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Definition
| group 18 gases - they are full and happy - they do not react usually also zero electronegativity |
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Term
| What are HALOGENS/ HALIDES? |
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Definition
| Group 17 fluorine, chlorine, etc |
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Term
| What 2 things did Rutherford learn from his GOLD FOIL experiment? |
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Definition
| atoms are mostly empty space and atoms have a tiny, dense nucleus |
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Term
| Which particle is negative? |
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Definition
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Term
| Which particles have the same mass? |
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Definition
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Term
| Which particle is positive? |
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Definition
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Term
| Which particle is neutral? |
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Definition
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Term
| Which side of the Periodic Table are metals usually found? |
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Definition
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Term
| Which side of the Periodic Table are nonmetals usually found on? |
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Definition
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Term
| What subatomic particle has almost no mass? |
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Definition
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Term
| how do you calculate the number of neutrons? |
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Definition
| mass number - atomic number |
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Term
| How do you know mass number? |
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Definition
| It is given in the notation |
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Term
| How do you find atomic number ? |
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Definition
| It is on the periodic table. |
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Term
| How do you find number of protons? |
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Definition
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Term
| How do you find the number of electrons? |
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Definition
| it is the same as protons. Atoms are neutral so positive and negative must balance. |
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Term
| How do you know if elements are isotropes? |
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Definition
| they have the same element symbol, same atomic number, but different mass and different neutrons |
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Term
| How do you know if elements are allotropes? |
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Definition
| They are the same element, but different formulas, shapes, structures, properties |
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Term
| Where do I find the ground state e- configuration? |
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Definition
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Term
| What is the excited state? |
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Definition
| when an e- has absorbed energy and jumped up a level. |
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Term
| What si the difference between quantitative and qualitatitve? |
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Definition
| quantitative is number data; qualititative is descriptive |
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Term
| What is the difference between an observation and an inference? |
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Definition
| Observations are facts gained from your 5 senses; inferences are your Ideas/thoughts about your observations |
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Term
| What are the 7 diatomics? |
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Definition
| H2,O2, N2, F2, Cl2, Br2, I2 |
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Term
| how do you calculate the number of neutrons? |
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Definition
| mass number - atomic number |
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Term
| Why are metals good for pots and pans? |
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Definition
| they conduct heat well , to cook the food evenly |
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Term
| Why are metals used for wires? |
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Definition
| metals are ductile and conduct electricity well because metals lose e- easily which allows electricity to flow |
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Term
| What is Ionization Energy? |
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Definition
| the amount of energy it takes to remove an electron |
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Term
| In Rutherford's experiment , MOST of the alpha particles went through UNDEFLECTED, this meant… |
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Definition
| that atoms were mostly empty space |
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Term
| In Rutherford's experiment, A FEW of the alpha particles were repelled backward and scattered, this meant… |
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Definition
| that atoms have a small dense core in the middle called the nucleus |
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