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| Highlight the Alkali Metals group on the periodic table. |
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Definition
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| Draw an arrow on the blank periodic table showing the direction of increasing ionization energy |
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Definition
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Term
| Highlight the Alkaline Earth Metals on the periodic table |
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Definition
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Term
| Highlight the Transition Metals on the periodic table |
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Definition
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Term
| Draw in the Metalloid staircase on the periodic table |
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Definition
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Term
| Highlight the Halogen group on the periodic table |
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Definition
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Term
| Highlight the Nobel Gases on the periodic table |
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Definition
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Term
| Describe the similarities and differences between atoms and elements |
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Definition
| Atom is a general term for particles that make up all matter. Elements are atoms with specific characteristics. So, Helium is an atom, but also an element with Noble Gas characteristics |
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Term
If elements are in the same period, they have the same number of .
If elements are in the same group they have the same number of . |
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Definition
| Atomic Orbitals, Valence Electrons |
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Term
| Electronegativity increases as you move to the right on the periodic table and decreases as you move down the periodic table. Evaulate this observation by applying principles of intermolecular forces. |
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Definition
Electronegativity increases as you move right because more electrons are added to the valence shell and more protons are added to the nucleus.This results in more proton-electron pairs, causing more attractive forces between electrons and protons.
Electronegativity decreases as you move down because more atomic orbitals are added, so the valence electrons are further away from the nucleus. This results in less attractive forces between valence electron(s) and protons because the distance between protons and electrons increases. |
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Term
| Draw an arrow on the blank periodic table showing the direction of increasing electronegativity |
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Definition
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Term
| Evaluate the relationship between ionization energy and electronegativity |
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Definition
| If it takes more energy to remove an electron from an atom (higher ionization energy) then the nucleus of that atom will have a strong attraction to valence electrons, causing a strong attraction to bonding electrons (higher electronegativity) |
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Term
| Create an imaginary element that would have the following characteristics: 1 unpaired electron, reactive with alkali and alkaline earth metals |
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Definition
| Students should create an element with the same characteristics of group 7 elements (F,Cl,Br, etc.) |
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Term
| Nitrogen can form only four bonds while Phosphorous commonly forms five bonds. Justify this observation (hint: consider differences in electron configuration) |
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Definition
Phosphorous:1s22s22p63s23p3
Nitrogen: 1s22s22p3
Phosphorous can exceed the octet rule because it is in the third period, and so has unfilled d-orbitals. Nitrogen cannot because it is in period 2 and cannot access the d-orbitals
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Term
| Noble gases are unlikely to form bonds with other atoms. Create an analogy that explains this property. |
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Definition
| Noble gases are "electron rich" (they have a full valence shell). This makes noble gases "happy," meaning that they do not want any more negative electrons. For this reason, noble gases are generally unreactive. |
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Term
| Draw an arrow(s) on the blank periodic table showing the direction of increasing atomic radii |
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Definition
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Term
| At room temperature, Cl2 is a gas, Br2 is a liquid, and I2 is a solid. Using your knowledge of intermolecular forces, create an explanation for this observation. |
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Definition
| Cl2 has a smaller radius than Br2, which has a smaller radius than I2. This means that I2 has greater intermolecular forces (London Dispersion Forces) based off of its surface area, which causes it to be a solid. |
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Term
| The periodic table is not the only way to organize the elements. Propose some other ways to list and categorize the elements. |
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Definition
| Students could organize by characteristics such as mass, alphabetization, melting point, boiling point, etc. |
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Term
| What are some properties of nonmetals? What are some properties of metals? |
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Definition
Nonmetals: poor conductors, brittle, lack luster, and gain electrons easily
Metals: good conductors, shiny, malleable, and lose electrons easily |
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Term
| Which circle could represent a chloride anion (Cl1-)?[image] |
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Definition
| Circle D. Chlorine is an anion, so it will gain electrons and increase in size |
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Term
| Anions have a charge and are larger/smaller than the original atoms? |
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Definition
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Term
| In what periodic table group does Element B belong?[image] |
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Definition
| Alkali metal (1 valence electron) and/or Group 1A |
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Term
Write the electron configuration for:
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Definition
Sodium: 1s22s22p63s1
Bromine: [Ar] 4s2 3d10 4p5
Oxygen: 1s22s22p4
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Term
| Element J is a metal and its chloride has the formula JCl2. What periodic table group does this element belong in? Justify your answer. |
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Definition
Group 2 (IIA)
The chemical formula shows that element J has a 2+charge, which places it in group 2, whose elements have two valence electrons and are metals. |
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Term
| Would the ion of Sodium be larger or smaller than the original atom? Why? |
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Definition
| Smaller. Sodium has a 1+ oxidation number, so it loses one electron, emptying the 3S orbital. |
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Term
| In an isotope, which part of the atom changes? Isotopes differ in atomic , not atomic number |
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Definition
Isotopes have a different number of neutrons than the original atom.
Isotopes differ in atomic mass, not atomic number. |
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Term
| Determine the number of protons, neutrons, and electrons in the Copper isotope Copper-64 |
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Definition
29 protons, 29 electrons, 35 neutrons
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Term
| Imagine that you encounter an alien from the planet Zygrot. Form an explanation of what matter is that would be easily understood by an organism completely unfamiliar with the periodic table and concepts of matter. |
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Definition
| Matter is that which occupies space and has mass. An effective response would include creative definitions of mass, space, and a general overview of atomic particles. |
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Term
| What element is in group 2 and period 4 of the periodic table? |
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Definition
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Term
| What is the only element that is a nonmetal and liquid at room temperature? |
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Definition
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