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Atoms
Chemistry
| Question | Answer |
|---|---|
| Atom. | The smallest unit of an element that maintains the properties of that element. |
| Element. | A pure substance that cannot be broken into simpler substances, composed of one type of atom. |
| Compound. | A substance made up of atoms of two or more elements that are chemically combined. |
| Ancient Greek's theory. | Over 2,000 years ago, viewed matter as being composed of the four elemental substances. (Water, earth, fire, and air), was later disproved. |
| Robert Boyle's theory. | 1600's, discovered the elements silver and gold, which led to the search for more elements, which disproved the Greek's concept. |
| Dalton's theory. | 1700's, all matter is composed of small particles called atoms, which cannot be subdivided (disproved), created, or destroyed, atoms of a given element are identical in their chemical and physical properties, atoms of different elements are dissimilar. |
| Dalton's theory continued. | Atoms of different elements have different properties, atoms of different elements combine in simple, whole number ratios to form compounds. |
| Law of Conservation of Mass. | Established by Dalton, in chemical reactions, atoms are combined, separated, or rearranged but never created, destroyed, or changed. |
| Planetary Model. | Established in the 1900's by Bohr, proposed model of the atom by showing a dense nucleus with electrons found in surrounding orbits. |
| What is the difference between the Plum Pudding Model and the Planetary Model? | The Planetary Model has a positive nucleus and electrons in orbit. |
| Wave Mechanical Model. | Has electrons in orbitals, which is the most probable location of electrons. |
| *Go over drawings of models* | WOAH |
| Who discovered the electron and how? | JJ Thompson with the Cathode Ray Tube. |
| How did JJ Thompson imagine the atom looked? | Negatively charged electrons in a positive fluid. |
| Who discovered the nucleus and how? | Rutherford, the gold foil experiment. |
| Explain the results of the gold foil experiment. | Most of the alpha particles went straight through, indicating that atoms are mostly empty space. However, some did deflect, proving that the nucleus is dense and positively charged. |
| Charge, mass, and location of protons. | Charge- +1 Mass- 1 amu Location- nucleus |
| Charge, mass, and location of neutrons. | Charge- 0 Mass- 1 amu Location- nucleus |
| Charge, mass, and location of electrons. | Charge- -1 Mass- 1/1836 amu (negligible) Location- orbitals |
| What does amu stand for and how was it established? | Atomic mass unit, based on 1/12 of a carbon-12 atom. |
| What is the function of a neutron? | To stabilize the nucleus. |
| What is the "fingerprint" of an element? | The atomic number. |
| What three things does the atomic number tell you? | Number of protons, nuclear charge, and number of electrons (if it's an atom). |
| What does the mass tell you? | Number of protons and neutrons combined (number of nucleons). |
| How many electrons does each principle energy level hold? | 1- 2 electrons 2- 8 electrons 3- 18 electrons 4- 32 electrons |
| The principle energy levels farther from the nucleus have ______ energy. | More. |
| Formula for speed of light. | Speed of light= wave length x frequency |
| At what rate does electromagnetic radiation travel through a vacuum of speed? | Speed of light=3 x 10 to the eighth power |
| What does C stand for? | Speed of light. |
| What does the upside down y stand for? | Wavelength. |
| What does the v stand for? | Frequency. |
| Wavelength and frequency are _____________ proportional. | Inversely. |
| Light emitted by an electron moving from a higher to lower energy level has a frequency ____________ proportional to the energy charge of the electron. | Directly. |
| Formula for energy of light. | Energy of light= "h" x frequency of light. |
| Formula for "h". (Which just serves as Plahck's Constant) | H= 6.63 x 10 to the negative 34th power (with the label js) |
| Electrons can move to different energy levels through gaining or losing _____________. | Energy. |
| Energy is lost/gained in __________ amounts. | Discrete. (You can't get/lose half of J) |
| What is the state called that electrons normally occupy? | The ground state. |
| What is the state called directly after an electron gets bombarded by a photon with higher energy? | The excited state. |
| The excited state of an electron is ______________. | Unstable. |
| How is energy released after the excited state? | Energy is released in the form of light and goes back to ground state. |
| Frequency. | Number of wave cycles in a given time to pass a given point. |
| Unit for frequency. | 1/sec. |
| Each element has a unique ___________ of light that occurs when reaching the ground state after the excited state. | Spectrum. |
| Purple has the __________ frequency. | Highest. |
| Red has the __________ frequency. | Lowest. |
| What does n stand for? | Principal Energy Level. |
| Wavelength. | Distance between two crests. |
| How many electrons, orbitals, and sub levels does n=1 have? | 2 electrons, one sublevel s with two electrons, one orbital. |
| How many electrons, orbitals, and sub levels does n=2 have? | 8 electrons, two sublevels, s with two and p with 6 electrons, three orbitals. |
| How many electrons, orbitals, and sub levels does n=3 have? | 18 electrons, three sublevels, s with 2, p with 6, and d with 10 electrons and five orbitals. |
| How many electrons, orbitals, and sub levels does n=4 have? | 32 electrons, 4 sublevels, s with 2, p with 6, d with 10, and f with 14 electrons and 7 orbitals. |
| Isoelectric. | Ions and Atoms that have the same electron configuration. |
| The farther away from the nucleus, the __________ the energy that the electron occupies. | Higher. |
| Difference in energy between two energy levels. | Quantum/Quanta. |
| Elements in the same family are located in the same ___________. | Column. |
| What is the same with all elements in a family and what does this determine? | Same number of valance electrons, which determines how a chemical reacts. |
| Members of the same group have similar ___________ ______________. | Chemical properties. |
| Elements in the same period are located in the same ____________. | Row. |
| What does the period number represent? | Number of occupied principle energy levels. |
| True or False: Properties of elements change as you go across the periodic table. | True. |
| Isotope. | Atoms of the same element that contain different numbers of neutrons. |
| Isotopes have different __________ _____________. | Mass numbers. |
| What does the atomic mass in decimal form tell us? | By looking at the whole number closest to the decimal, we can determine which isotope is most abundant. |
| Atomic mass. | Weighted average mass of an atom's naturally occurring isotopes. |
Created by:
emarciante10
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