Chemistry Chapter 6 Guided Reading Questions.
1. How did John Newlands arrange the known elements? A: By periodicity: the “law of octaves,” that every eight elements have similar chemical and physical properties.
2. . What pattern did the elements in Newlands arrangement follow? A: again, the “law of octaves,” every eight elements had similar properties (see the worksheet packet, front page)
3. **skip** (Meyer helped Mendeleev)
4. What is Mendeleev credited for first developing? A: The first periodic table, arranged by atomic *MASS
5. Why was his periodic table widely accepted? A: Elements were found to be ordered by increasing atomic mass had similar chemical and physical properties AND he could predict patterns of behavior in unknown elements also
6. What was found to be wrong with Mendeleev’s periodic table? A: The increasing atomic mass was sometimes not predictable of all properties because the Masses are inconsistent (we now know those are due to isotopes of elements)
7. MOSELEY: Arranged periodic table according to *increasing atomic number.
8. Periodic law: When elements are arranged according to increasing atomic number, (originally, atomic Masses by Mendeleev), fall into recurring groups, so that elements with similar physical and chemical properties occur at regular intervals, in other words, relationships and similarities in their properties can be observed.
9. Groups are the VERTICAL COLUMNS (up and down) on the periodic table. Elements in the same group have similar chemical properties. PERIODS ARE THE ROWS.
10. Representative elements are the *s and p block elements, groups 1,2 and 13-18. Transition elements are the transition metals in the d-block, groups 3-12.
11. Metals are elements that make up 75% of the periodic table. They are shiny, hard solids that are ducticle, can conduct electricity, are malleable (bendable to be used for materials such as for building and construction).
12. Nonmetals are at the far right side of the periodic table (in groups 14-18) and are mostly gases. Some are liquids, some are brittle solids (non conductors of electricity) such as sulfur and phosphorus.
13. Metalloids are elements that have properties of both metals and nonmetals.
Section 2: Classification of the Elements
1. What are valence electrons? A: The electrons in the outermost s and p energy level of an atom. Atoms in the same group in the s and p blocks have the same number of valence electrons (1,2 have 1,2 valence electrons, respectively, and 13-18 have 3 – 8). Elements in the same group have similar chemical properties.
2. What is the relationship between valence electrons and period on the periodic table? A: The period number indicates the main/principle energy level the valence electrons are in.
3. Atoms in the same group in the s and p blocks have the same number of valence electrons (1,2 have 1,2 valence electrons, respectively, and 13-18 have 3 – 8). Elements in the same group have similar chemical properties.
4. S-block elements are groups 1 and 2, the alkali metals and the alkaline earth metals
5. P block elements contain metals, metalloids, and all nonmetals including halogens and noble gases.
6. D-block are the transition metals
7. F-block are the inner transition metals
Section 3: Periodic Trends
USE YOUR POWER POINT AND THE NOTES FROM TODAY