Question

1. what is the order of the periodic chart based on 2. name the alkali metals 3. name the alkaline earth metals 4. know where to find transitional metals 5. know where to find the noble gasses 6. who created the first periodic chart 7. know how to find the halogens 8. know how to differentiate metals, nonmetals and metalloids 9. know the characteristics of all three 10. atoms of the same group have the same number of 11. know how to locate the protons of an element 12. know how to find the electrons of an element 13. know how to find the neutrons of an element 14. columns are called what 15. rows are called what 16. each row you add another ________ to the element 17. as you move from left to right on the periodic chart the number of ______ increases 18. what is an ion 19. when an atom loses an electron, it becomes ______ 20. when an atom gains an electron, it becomes ______ 21. group 7 would form a (+ or -) ion? 22. most elements are (metals, nonmetals or metalloids) 23. the most abundant form of element is (metal, nonmetal or metalloid) 24. why is potassium highly reactive? 25. what is ionization 26. describe atomic radii 27. describe ionic radii 28. describe electronegativity 29. describe ionization energy 30. noble gasses have a ______ outer shell and makes them ________ atoms 31. define proton, neutron and electron (charge, mass, location) 32. which groups will form positive ions and which groups will form negative ions 33. lithium would have a (+ or -) charge 34. know how to draw bohr’s model 35. know how to draw electron dot diagram

Explanation:

1. The periodic chart is ordered by atomic number.
2. Alkali metals are lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), francium (Fr).
3. Alkaline - earth metals are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), radium (Ra).
4. Transition metals are in groups 3 - 12.
5. Noble gases are in group 18.
6. Dmitri Mendeleev created the first periodic chart.
7. Halogens are in group 17.
8. Metals are typically shiny, good conductors of heat and electricity; non - metals are poor conductors; metalloids have intermediate properties.
9. Metals are malleable and ductile, non - metals are brittle, and metalloids have some metallic and non - metallic properties.
10. Atoms of the same group have the same number of valence electrons.
11. The number of protons is equal to the atomic number of the element.
12. In a neutral atom, the number of electrons is equal to the number of protons.
13. Neutrons = Mass number - Atomic number.
14. Columns are called groups.
15. Rows are called periods.
16. Each row you add another energy level to the element.
17. As you move from left to right on the periodic chart the number of protons (atomic number) increases.
18. An ion is an atom or molecule with a net electric charge.
19. When an atom loses an electron, it becomes a positive ion (cation).
20. When an atom gains an electron, it becomes a negative ion (anion).
21. Group 7 elements form negative ions (-).
22. Most elements are metals.
23. The most abundant form of elements in the Earth's crust is non - metals (oxygen is the most abundant element overall).
24. Potassium is highly reactive because it has one valence electron and readily donates it to achieve a stable electron configuration.
25. Ionization is the process of converting an atom or molecule into an ion by adding or removing electrons.
26. Atomic radii is the distance from the nucleus to the outermost electron shell of an atom.
27. Ionic radii is the radius of an ion, which can be larger or smaller than the parent atom depending on whether it is a cation or anion.
28. Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.
29. Ionization energy is the energy required to remove an electron from an atom or ion in the gaseous state.
30. Noble gases have a full outer shell and are stable atoms.
31. A proton has a positive charge (+1), mass of approximately 1 amu, and is located in the nucleus; a neutron has no charge, mass of approximately 1 amu, and is located in the nucleus; an electron has a negative charge (- 1), very small mass, and is located in the electron cloud.
32. Metals (groups 1 - 2 and some in transition metals) form positive ions; non - metals (groups 15 - 17) form negative ions.
33. Lithium has a + charge.
34. To draw Bohr's model, represent the nucleus with protons and neutrons, and electrons in circular orbits around the nucleus.
35. To draw an electron - dot diagram, represent the element symbol and place dots around it to represent the valence electrons.

Answer:

1. By atomic number.
2. Lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), francium (Fr).
3. Beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), radium (Ra).
4. Groups 3 - 12.
5. Group 18.
6. Dmitri Mendeleev.
7. Group 17.
8. Metals are shiny, good conductors; non - metals are poor conductors; metalloids have intermediate properties.
9. Metals are malleable/ductile, non - metals are brittle, metalloids have intermediate properties.
10. Valence electrons.
11. Equal to the atomic number.
12. Equal to the number of protons in a neutral atom.
13. Neutrons = Mass number - Atomic number.
14. Groups.
15. Periods.
16. Energy level.
17. Protons (atomic number).
18. An atom or molecule with a net electric charge.
19. Positive ion (cation).
20. Negative ion (anion).
21. - (negative).
22. Metals.
23. Non - metals.
24. It has one valence electron and readily donates it.
25. The process of converting an atom or molecule into an ion by adding or removing electrons.
26. Distance from nucleus to outermost electron shell.
27. Radius of an ion.
28. Measure of an atom's ability to attract electrons in a chemical bond.
29. Energy required to remove an electron from an atom or ion in the gaseous state.
30. Full; stable.
31. Proton: +1 charge, ~1 amu, in nucleus; Neutron: 0 charge, ~1 amu, in nucleus; Electron: - 1 charge, very small mass, in electron cloud.
32. Metals (groups 1 - 2 and some transition metals) form positive ions; non - metals (groups 15 - 17) form negative ions.
33. + (positive).
34. Represent nucleus with protons/neutrons, electrons in circular orbits.
35. Represent element symbol, place dots for valence electrons.