1 / 60

Regents Chemistry

Regents Chemistry. Topic 2 The Periodic Table and Formulas / Equations. Regents Chemistry. Introduction to the Table Groups and Families Elements of Metals, Nonmetals and Metalloids. Recap. The nucleus contains protons and neutrons. Nucleus. Electrons surround the

susannej
Download Presentation

Regents Chemistry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Regents Chemistry Topic 2 The Periodic Table and Formulas / Equations

  2. Regents Chemistry • Introduction to the Table • Groups and Families • Elements of Metals, Nonmetals and Metalloids

  3. Recap • The nucleus contains • protons and neutrons Nucleus • Electrons surround the • nucleus in a “cloud” • Atomic number is the • number of protons • Atomic mass is the • sum of protons and • neutrons electrons

  4. The Periodic Table • The periodic table is arranged according to Atomic Number • The first table, by Russian chemist Dmitri Mendeleev, was arranged by atomic mass, but this was not accurate • Current arrangement shows many important trends..

  5. Rows and Columns

  6. Divisions of the Periodic Table • Metals • Alkali metals • Alkaline earth metals • Transition Metals • Metalloids • Nonmetals • Halogens • Nobel gases

  7. Periodic Table

  8. Physical Properties of Metals • Efficient conduction of heat and electricity • Malleability (they can be hammered into • thin sheets • 3. Ductility (they can be pulled into wires) • 4. A lustrous (shiny) appearance

  9. Natural States of Elements • Most of the matter around us consists of mixtures • Mixtures contain compounds • Atoms of individual elements are not often found in nature in pure form • Some exceptions: gold, platinum and silver • Also noble gases – do not combine readily • Ex; Helium gas in underground deposits

  10. Elements after Separation.. • After we use a chemical process to separate the elements in a compound, we find the elements to be: • Monoatomic atoms– only (1) atom of the element • Diatomic molecules– (2) atoms bonded together

  11. Examples • Argon (noble gas) • Nitrogen and • oxygen

  12. Natural Physical States • Metals are solids at 25 C • Noble gases are gas at room 25 C and are individual atoms • Several others are gases and diatomic at 25 C – (H2, N2, O2, F2, Cl2) • Only two elements are liquids at 25 C • Bromine and Mercury

  13. Elements can have different forms… • Solid metals differ from solid non-metals • In fact, different forms of the same element can occur • These are called allotropes • Ex: Carbon • Diamond (very hard) • Graphite (soft) • Buckministerfullerene (newly discovered) End

  14. Regents Chemistry • Information on the Table • Average Atomic Mass • Atomic Number • Isotopes

  15. Regents Chemistry • Periodic Table Bingo

  16. Regents Chemistry • Ions and Oxidation States

  17. **Change ending of parent name to -ide and add word - ion**

  18. Cloride Anion

  19. ***Keep parent name and add word - ion***

  20. Sodium Cation

  21. Ionic charges from Periodic Table See pg. 112

  22. Writing out ionic charges Gain e- Sodium ion Lose e- Magnesium ion

  23. Ionic Compounds • Combination of cation and anion • Write cation first and anion second • When combining, we must consider electrical charge • Ions combine in such a way to make a zero net charge Total charge of cations Total charge of anion Zero net charge + =

  24. Examples

  25. More Examples... Dissolving Ionic CompoundsVideo Does this work? = worksheet

  26. Regents Chemistry • Chemical Nomenclature

  27. Naming Compounds • Common names were originally developed to name compounds • Ex: Epsom salts, milk of magnesia, gypsum and laughing gas • Too many common names..a system had to be developed!

  28. Naming Compounds • Binary compounds – compounds that are composed of two elements • We will examine two classes of binary compounds • 1. Compounds that contain a metal and a nonmetal • 2. Compounds that contain two nonmetals

  29. Naming Binary Ionic Compounds • Binary ionic compounds result when a metal combines with a nonmetal • The metal loses electrons as the nonmetal gains electrons • The result is a positive cation (the metal) and a negative anion (the nonmetal) • In naming ionic compounds, we simply name the ions

  30. Naming Binary Ionic Compounds • We will learn how to name two types of ionic compounds (polyatomic ion naming will come later) • Type I compounds – The metal is present in only one type of cation - look at periodic table! • Ex: Na+, K+, Ca2+, Al3+ • Type II compounds – The metal present can form two (or more) cations that have different charges - look at periodic table! • Ex: Cr2+, Cr3+, Cu+, Cu2+

  31. Some Common Examples

  32. Naming Rules for Type I Ionic • 1. The cation is always named first and the anion second • 2. A simple cation (obtained from a single atom) takes its name from the name of the element. • Ex: Na+ Sodium ion • 3. A simple anion (obtained from a single atom) is named by taking the first part of the elemental name and adding – ide • Ex: F- Fluoride ion

  33. Examples • Name the following compounds • NaCl • KI • CaS CLICK TO REVEAL ANSWERS sodium chloride potassium iodide STOP worksheet calcium sulfide

  34. Regents Chemistry • Naming Type II Compounds

  35. Naming Type II compounds • Type II compounds – The metal present can form two (or more) cations that have different charges - look at periodic table! • Ex: Cr2+, Cr3+, Cu+, Cu2+ • We cannot only look at the periodic table to determine the charge…we must determine the charge according to the chemical formula

  36. Determing the correct charge • All compounds must be electrically neutral..so • we use the charge of the anion to determine the charge of the cation…and multiply the charges by the number of atoms to determine the overall net charge

  37. Example CuCl Cl comes in as Cl- : -1 x 1 Cl ion = -1 Cu must come in as a +1 :+1 x 1 Cu ion = +1 -1 + +1 = 0 , the charges balance Copper (I) Chloride

  38. Naming Type II Rules • Use the same system of naming as Type I binary compounds..except • add the following after the cation depending on the cation’s charge (I) +1 (V) +5 (II) +2 (VI) +6 (III) +3 (VII) +7 (IV) +4

  39. Practice • HgO • Fe2O3 Mercury (II) Oxide Iron (III) Oxide Worksheet

  40. Regents Chemistry • Naming Type III Binary Compounds Non-metal to non-metal

  41. Type III Binary Compounds • Type III Binary Compounds - are compounds that contain only nonmetals participating in covalent bonds (sharing of electrons)

  42. Rules for Naming Type III • 1. The first element in the formula is named first, and the full element name is used • 2. The second element is named as though it were an anion (-ide ending) • 3. Prefixes are used to denote the numbers of atoms present. • 4. The prefix mono is never used for naming the first element

  43. Prefixes for Naming Type III PREFIX NUMBER INDICATED mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8

  44. Practice • BF3 • NO • N2O5 • carbon tetrachloride boron trifluoride nitrogen monoxide dinitrogen pentoxide CCl4 worksheet

  45. Regents Chemistry • Polyatomic Ion Compound Nomenclature

  46. What’s a polyatomic ion? • A polyatomic ion consists of two or more elements bonded together that posess an overall net charge that can be used to form an ionic bond with a metal cation • We looked at some of these! SO42-

More Related