Introduction to Periodic Table (Science)

All about the Elements

1. READY FOR SECOND QUARTER?

2. Introduction to the Periodic Table Atomic Number ● Symbol ● Atomic Weight Element ● Compound ● Mixture

3. I am Dmitri Mendeleev! I made the PERIODIC TABLE !

4. Russian Chemist who first published the first version of a systematically organized periodic table of elements. This table was arranged in order of increasing atomic mass and was the basis of the currently used periodic table. He organized the elements into columns called groups or families and rows called periods and series. This arrangement observed what is now known as periodic law , which asserts that when elements are arranged according to increasing atomic mass, their properties will follow a periodic pattern.

5. German chemist who recognized the similarities in the chemical properties of some triads of elements, upon which observation he established his law of triads. However, the limited number of element triads could not support his hypothesis. Johann Wolfgang Döbereiner

6. German Chemist who published a periodic table in 1864 where there then known 44 elements were organized based on the valency of the elements. He later published in 1870 an improved version that related atomic volume and atomic number. LOTHAR MEYER

7. Proposed the laws of octaves which recognized the periodic properties of every eighth element in his list. JOHN AR NEWLANDS

8. What is PERIODIC TABLE?

9. What is the PERIODIC TABLE? Shows all known elements in the universe. Organizes the elements by chemical properties.

10. How do you read the PERIODIC TABLE?

11. What is the ATOMIC NUMBER? The number of protons found in the nucleus of an atom Or The number of electrons surrounding the nucleus of an atom.

12. What is the SYMBOL? An abbreviation of the element name.

13. What is the ATOMIC WEIGHT? The number of protons and neutrons in the nucleus of an atom.

14. How do I find the number of protons, electrons, and neutrons in an element using the periodic table? # of PROTONS = ATOMIC NUMBER # of ELECTRONS = ATOMIC NUMBER # of NEUTRONS = ATOMIC _ ATOMIC WEIGHT NUMBER

15. How do I find the number of protons, electrons, and neutrons in an element using the periodic table? p n e A Z Isotopes 6 6 6 6 12

16. How do I find the number of protons, electrons, and neutrons in an element using the periodic table? Number of Electrons = 56 Number of Neutrons = 14 Name of Element = ______ Mass Number = ______ Number of Protons = 24 Number of Neutrons = 14 Name of Element = ______ A = ______ Z = 50 Number of Neutrons = 69 Name of Element = ______ Mass Number = ______ Number of Electrons = 34 Number of Neutrons = 45 Name of Element = ______ Mass Number = ______

17. Elements, Compounds, and Mixtures

18. What is an ELEMENT? A substance composed of a single kind of atom. Cannot be broken down into another substance by chemical or physical means.

19. What is a COMPOUND? A substance in which two or more different elements are CHEMICALLY bonded together.

20. What is a MIXTURE? Two or more substances that are mixed together but are NOT chemically bonded.

21. Element, Compound or Mixture?

22. Element, Compound or Mixture?

23. Element, Compound or Mixture?

24. Element, Compound or Mixture?

25. Element, Compound or Mixture?

26. Element, Compound or Mixture?

27. The modern periodic table has 118 elements officially recognized by the International Union of Pure and Applied Chemistry (IUPAC). These elements are arranged in the periodic table in a way that they can easily be classified and identified. The A group (in longer columns) are classified as representative elements or main group elements; the B group elements (in shorter columns) are called transition elements.   Elements in the periodic table are also labeled vertically in groups or families, and horizontally in periods or series.

28. Groups and periods

29. 1. ALKALI METALS (GROUP 1A) They have only one electron in their valence shell (n s 1 ), which makes them very reactive because they can easily lose this electron to form their ions with a charge of +1.

30. 2. ALKALINE EARTH METALS (GROUP IIA) They have two valence electrons (n s 2 ), which they can lose to form +2 ions. These metals are also silver-colored and soft, with low densities, and melting and boiling points. They also react with water to form strongly alkaline hydroxides.

31. 3. TRANSITION METALS These are “typical” metals Middle “chunk” of periodic table. Group III to XII .

32. 4. OTHER GROUPS a. Group 3A (Boron Group) b. Group 4A (Carbon Group) c. Group 5A (Prictogens or Nitrogen Group) d. Group 6 A (Chalcogens or Oxygen Group) e. Group 7 A (Halogens)

33. 5. HALOGENS Most reactive non metals. Reacts with metals to form salt. Group 17 of Periodic Table.

34. 6. GROUP 8A (NOBLE GASES) Considered as non metals. The noble gases are relatively inert; they rarely form compounds with other elements. They can exist as monatomic gases. Group 18 of the periodic table of element.

35. NEIL BOHR’S ATOMIC mODEL

36. Bohr’s Model of the Atom In 1913, Niels Bohr, a Danish physicist working in Rutherford’s laboratory, proposed a quantum model for the hydrogen atom that seemed to answer this question. This model correctly predicted the frequency lines in hydrogen’s atomic emission spectrum.

37. The lowest allowable energy state of an atom is called its ground state . When an atom gains energy, it is in an excited state.

38. Bohr’s Model of the Atom Each orbit was given a number, called the quantum number . Bohr orbits are like steps of a ladder, each at a specific distance from the nucleus and each at a specific energy.

39. QUANTUM MECHANICAL MODEL OF ATOM

40. Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus.

41. Pz