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Unit 2 Lesson 2 Test
| Question | Answer |
|---|---|
| How did Henry Moseley arrange the elements in the periodic table? | By atomic number and by properties |
| How many groups make up the current Periodic table? | 18 |
| Which side of the table primarily has the nonmetals (in comparison to the stair-step line)? | The right side |
| Lithium is classified as.......? | Alkali Metal |
| Platinum is classified as........? | Transition metal |
| List two other element with similar chemical properties compared to iron. | Ruthenium and Osmium |
| Why do Alkali Metals all share the same physical and chemical properties? | They are all in the same group and only have one valence electron. |
| How many valence electrons do elements in group 13 have? | 3 |
| What is the name of the group that has 8 valence electrons? | Noble Gases/ Group 18 |
| How does the shielding effect change the ionization energy in a group (top to bottom) of metals? | The shielding effect gets smaller as it goes down the elements in the group. |
| Do metals or nonmetals have higher ionization energy? | Nonmetals |
| Which atom would require more ionization energy to remove a valence electron: NA or FR? | Na because they attract electrons because they have less energy groups so the electrons are closer to the nucleus, which means it will be harder to pull away. Francium is so far that the electron is easy to take off. |
| How is an Ion formed? | When an atom gains or loses electrons |
| Which nonmetal is the most reactive? | Fluorine because they attract and really want another element, and since the energy levels are so small, it is easier to attract them. |
| How does the atomic radius change in a group from top to bottom? | It gets bigger from the top to bottom |
| How is the atomic radius of bromine different from the radius of Iodine? | Bromine has a smaller radius than Iodine does |
| How many valence electrons do elements want to have? | 8, or 2 for helium |
| How did Mendeleev organize the elements on the periodic table in 1869? | Elements were organized by increasing atomic mass and properties. |
| How was the organization of the elements on the periodic table changed in 1913? | Henry Moseley arranged the elements by increasing atomic number and properties. |
| How are “periods” and “groups” arranged in the periodic table? What do they communicate? | Periods = Rows (increasing atomic number. Group = Column (same # of VE and similar properties) |
| Name of group 1 elements? | alkali metals |
| Name of group 2 elements? | alkaline earth metals |
| Where are the transition metals? | groups 3-12 |
| Name for the following elements? Al, Ga, In, Il, Nh, Sn, Pb, Fl, Bi, Mc, Po, Lv | post-transition metals |
| How many valence electrons do elements want to have? | 8 valence (just like the noble gases) *possibly 2 VE like helium* |
| How would an element from group 2 react with an element from group 16 to have VE like the noble gases? | Group 2 element (lose 2 electrons) Group 16 element (gain 2 electrons) |
| How is the atomic radius measured? | half the distance between nuclei of identical atoms |
| Compare the atomic radius of sodium to that of aluminum. | Na has larger radius than Al (aluminum’s electrons are pulled in more tightly) |
| Compare the atomic radius of chlorine to that of iodine. | Iodine has a larger radius (higher energy level and shielding effect) |
| How does the atomic radius change in a period from left to right? | the radius gets smaller from left to right in a period (more positive and negative charge in same area *more attraction*) |
| How does the atomic radius change in a group from top to bottom? | the radius gets bigger from top to bottom (add more/higher energy levels and shielding effect) |
| Which metal has the largest radius and is most reactive? | Francium |
| Which nonmetal has the smallest radius and is the most reactive? | Fluorine |
| Why do reactive metals have a large radius, but reactive nonmetals have a small radius? | metals: give away electrons (those farther from the nucleus are more likely to leave - less attraction) nonmetals: gain electrons (there is more attraction for electrons in smaller energy levels close to the nucleus) |
| How is an ion formed? | gain or lose electrons (an ion is a charged atom) |
| Which atom would require more ionization energy to remove a valence electron: Li or Cs? | Li |
| How does ionization energy change across a period from left to right? | increase from left to right |
| How does ionization energy change from the top of a group to the bottom? | decrease from top to bottom |
| Do metals or nonmetals have a higher ionization energy? | nonmetals |
| How can ionization energy be used as a measure of chemical reactivity for metals and nonmetals? | metals: low ionization energy = high reactivity nonmetals: high ionization energy = high reactivity (does not include noble gases) |
| How does the shielding effect change the ionization energy in a group (top to bottom) of metals? | the shielding effect decreases the ionization energy |
| How does the shielding effect change the ionization energy in a group (top to bottom) of nonmetals? | the shielding effect decreases the ionization energy |
| Is electronegativity about attracting electrons or removing electrons? | attracting electrons |
| Which has the lower electronegativity B or F? | B Boron |
| Which has the higher electronegativity N or Bi? | N Nitrogen |
| What is the period trend for electronegativity? | electronegativity increases from left to right |
| What is the group trend for electronegativity? | electronegativity decreases from top to bottom |
| How does the trend in electronegativity in the periodic table compare with the trend in atomic radii? | opposite trends from left to right: EN increases, Radii decrease from top to bottom: EN decreases, Radii increase |
| How does the trend in electronegativity in the periodic table compare with the trend in ionization energy? | same trends from left to right: EN increases, IE increases from top to bottom: EN decreases, IE decreases |
Created by:
ldalton
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