Periodic Table Study Guide - Weebly



Periodic Table Study Guide answer key

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1. How did Dobreiner arrange the periodic table? He grouped elements in groups of 3s or triads

2. How did Mendeleev arrange the periodic table and what was unique about him? He grouped elements according to increasing mass and according to repeating properties

3. Why was Moseley significant to the periodic table? He grouped elements according to increasing atomic number and according to their chemical properties

4. What is the modern periodic law? Physical and chemical properties of elements repeat in a regular pattern when they are arranged in order of increasing atomic number.

Period = horizontal row

Group/Family = vertical column

5. Where are metals located on the periodic table? All elements to the left of the stair step/zig zag line. What are their properties? Malleable, ductile, good conductors of heat and electricity, shiny. All have a + charge and are solids at room temperature (except mercury, which is a liquid at room temperature). High melting point.

6. Where are nonmetals located on the periodic table? All elements to the right of the stair step/zig zag line What are their properties? Brittle, dull, not good conductors of heat and electricity. All have a (-) charge and are usually a gas at room temperature. Low melting point

7. Where are the metalloids? The elements in the stair step, between the metals and non-metals. What are their properties? Properties of both metals and non-metals, used as semi-conductors: they are: boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb),tellurium (Te), polonium (Po) and astatine (At) 

8. Where are the alkali metals? In the first column of the periodic table What are their properties? Highly reactive, have one valance electron, gain a +1 charge when they lose 1 electron to become stable, all metals (hydrogen is not an alkali metal, however it is in the first column)

9. Where are the alkaline earth metals? In the second column of the periodic table. What are their properties? Very reactive, but not as reactive as the alkali metals. They have 2 valence electrons, gain a +2 charge when they lose 2 electrons to become stable, all metals

10. Where are the halogens? Column 17 or 7A What are their properties? Highly reactive non-metals, have 7 valence electrons, gain a -1 charge when they gain an electron to become stable. Their names all end in ine

11. Where are the noble gases? In the last column of the periodic table, also called goup 8A, 18 or 0 What are their properties? Have 8 valence electrons, no charge, do not react or bond with other elements. They are stable. All are gases at room temperature

12. Where are the transition metals? Group D (the middle of the periodic table). What are their properties? The same properties as metals, however they will take on the charge required to bond with another element. This is done by losing the number of valence electrons that the nonmetal it is bonding with needs. Example: Fe will have a +1 charge if it bonds with Cl that needs 1 electron to be stable, but it will have a +2 charge when it bonds with O which needs 2 electrons to be stable.

13. Where are the lanthanide metals? Lanthanides are found in the first energy level of the F sublevel, they fit into the periodic table after Lanthinium in the next to the last energy level of the D sublevel.

14. Where are the actinide metals? Actinide metals are found in the second energy level of the F sublevel, they fit into the periodic table after Actinium in the last energy level of the D sublevel.

15. What are the properties of hydrogen? Hydrogen is a highly reactive nonmetal gas. It has only one valence electron and will share electrons with another nonmetal to become stable.

16. What are the oxidation numbers for each group? IA or 1 has a +1 charge, IIA or 2 has a +2 charge, IIIA or 13 has a +3 charge, IVA or 14 has a +4 or a -4 charge, VA or 15 has a -3 charge, VIA or 16 has a -2 charge, VIIA has 17 has a -1 charge, and VIII or 18 has a 0 charge. The transition metals usually have a +2 charge, but it can be different depending on what they bond with.

17. What is the octet rule? Atoms are stable with 8 valence electrons in their outer most energy level.

18. Do metals “like” to gain or lose electrons? Lose electrons (because it takes less energy to lose less than to gain more.)

19. Do nonmetals “like” to gain or lose electrons? Gain electrons (because it takes less energy to gain less than to lose more)

20. What is atomic radius? The distance from the center of one atom to the center of another atom of the same kind.

21. What is the trend for atomic radius as you go down a group? The atomic radius increases as you move down the periodic table WHY? Because there are more energy levels What is the trend for atomic radius as you go across (L(R) a row? There are more protons pulling on the electrons bring them closer to the nucleus making the radius smaller.WHY? when the electrons are pulled closer to the nucleus by more protons it decreases the size of the atom.

22. What is a cation? An atom (metal) that has lost electrons and has become + charged Does a cation have a bigger or smaller radius than a neutral atom? Smaller because it has lost electrons.

23. What is an anion? An atom (non-metal) gains electrons and has a -charge. Does an anion have a bigger or smaller radius than a neutral atom? Bigger because there are now more electrons.

24. What is the most active metal? Francium Why? More energy levels and it is very close to being like a noble gas (only needs to lose 1 electron) (farthest to the bottom and left of the periodic table.) The farther from the nucleus the easier it is to lose electrons.

25. What is the trend for the reactivity of metals? As you move from left to right reactivity becomes less, as you move from top to bottom reactivity becomes greater.

26. What is the most active nonmetal? FluorineWhy? Nonmetals gain electrons and the closer an electron is to the nucleus of an atom the stronger the pull, so the top right would be the most active nonmetal. The closer to the nucleus an electron is the easier it is to be pulled in or gained.

27. What is the trend for the reactivity of nonmetals? Nonmetals are more reactive when they are closest to being a noble gas and have less energy levels. Top right.

28. What is ionization energy? The amount of energy it takes to remove an electron from an atom.What is the trend for ionization energy? as you move from left to right and from bottom to top ionization energy becomes greater.

29. What is electronegativity? The ability for a compound to gain electrons What is the trend for electronegativity? As you move from left to right and bottom to top the electronegativity becomes greater

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