1. IPC 03A Atoms & Elements

2. Atomic Structure History: John Dalton Dalton’s Atomic Theory: Proposed that elements are _____________________________ identical, indivisible particles called ___________________. The name “atom” comes from

3. J.J. Thomson “Plum Pudding” Model He said the atom had _____________ (raisins) immersed in a sea of ______________ ___________________ _(pudding).

4. J.J Thomson’s Cathode Ray Tube Experiment: He concluded that the _________________ were made up of very small _______________ charged particles, which he named __________

5. Ernest Rutherford “Gold Foil” Experiment Discovered the ________________________ and that the atom is mostly _____________.

6. Rutherford’s Expectation (assuming the plum pudding model) Rutherford expected ______ ______________ particles to go ______________ the atom like in this picture.

7. Rutherford’s Actual Results Instead, Rutherford observed that some of the __________ particles bounced _____________; thus, he concluded there was a ________________ ____________________ nucleus.

8. Niels Bohr “___________________” of the Atom Nucleus is in the __________. Electrons orbit the ____________.

9. Erwin Schrodinger “_______________________” The ___________ represents the probable ______________ of an __________.

10. James Chadwick Discovered the ____________ There was still __________ _____________ from the atom. Chadwick solved the problem by discovering the final subatomic particle, the __________________. Jimmy Neutron

11. Exposing Scientist’s Contributions Atomic Theory John Dalton J.J. Thompson RutherfordJ. ChadwickNiels BohrSchrodinger

12. Atoms consist of three main Subatomic Particles Atomic mass unit (amu) = ___________ the mass of a __________________________. Protons p+ Electrons e - Neutrons n 0 Mass Charge

13. Structure of The Atom ____________ is small, dense, and _______ ____________ charged. ___________ are located outside the nucleus in an ________ __________

14. Forces Within The Atom Electromagnetic Forces keep the electrons in _____________around the nucleus. The negatively charged _________________ are _____________ to the positively charged _____________ in the nucleus. Strong Nuclear Forces hold the _______________together by opposing the force of _____________ between the positive charged ____________ so the nucleus won’t break apart. Only acts on very short distances.

15. Chemical Symbols Elements are the simplest pure substance that _______________________ ____________________. Chemical symbols are an _________________ of the element’s name. The first letter is ALWAYS ____________ and the second letter is ALWAYS __________! ElementSymbolOrigin CopperCuCuprium GoldAuAurium IronFeFerrium LeadPbPlumbum PotassiumKKalium SilverAgArgentum SodiumNaNatrium TinSnStannum

16. An Element- contains one type of atom with a unique number of ______________________. oToT he _________________ determines the element. oEoE x: Carbon has ____ protons. oIoI f you _____________ the # of protons, you change the _____________________. oEoE x: Nitrogen has ____ protons. Neutral Atoms have the __________ # of electrons as protons. Ex: neutral Carbon has 6 ________ and 6 ________

17. Element Notation Mass Number (M) – –Found in the ______________ and makes of up _______ of the atom’s ___________ (99.99%). Atomic Number (A) - number of _____________________ –Determines the ____________. X M A

18. Example: Carbon-12 1) What is the atomic number of Carbon? 2) What is the mass number of Carbon? C 12 6

19. Isotopes AA toms with the SS ame _____________________(same atomic #) DD ifferent _______________________________ DD ifferent ______________________________

20. Sodium Isotopes 1) Atomic number? 2) Mass number? 3) No. of Neutrons? 4) Atomic number? 5) Mass number? 6) No of Neutrons?

21. Hydrogen Isotopes Hydrogen-1 (______________) Hydrogen-2 (_______________) Hydrogen-3 (______________)

22. Hydrogen Isotopes Fill in the #protons, #electrons, & #neutrons: Mass numberNo. of protons No. of electrons No. of neutrons Hydrogen-1 Hydrogen-2 Hydrogen-3

23. Atomic Mass – is the _______________________ of all the element’s natural ________________ The most common isotope will have a ________ __________________ of the atomic mass rounded to a ____________________number. Atomic number = Atomic Mass = The most common isotope of silver is ______________.

24. Mendeleev’s Periodic Table Dimitri Mendeleev – organized information about all the known elements by

25. Groups & Periods Groups (Families) have similar properties and go down on the periodic table. There are Periods go across on the periodic table. There are

26. Identify the element in: Group 2 (IIA), period 4 Group 17 (VIIA), period 5 Group 11, period 4 Look at the Periodic Table:

27. Metals, Nonmetals, & Metalloids

28. Properties of metals and nonmetals Metalloids have both metallic and nonmetallic characteristics – along the staircase. Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Astatine MetalsNonmetals Luster (shiny silver-gray, gold, copper) ___________________ (all different colors) Malleable (hammered) Ductile (drawn into thin wire) __________Melting Points_________Melting Points ____________Conductors of heat & electricity _________ Conductors of heat & electricity ________________ electrons____________ electrons Silicon is used in computer chips because conduct electricity (metals) yet insulate (nonmetals).

29. Energy Levels in an Atom Electrons occupy ________ around the _________. Each energy level can hold up to ____ electrons where n = the _____________ The farther away an electron is, the higher the energy it possesses.

30. Electrons in Energy Levels 1.What is the most common isotope? 2.How many protons? 3.How many electrons? 4.How many neutrons? 5.How many electrons in the 1 st energy level? 6.How many electrons in the 2 nd energy level? 7.How many electrons in the 3 rd energy level? Cl 35.45 17

31. Absorption of Energy The __________________ absorbs enough __________________ causing the electron to be _________________ and “_____________” to a _____________________________energy level.

32. Emission of Energy The electron _______________ when it falls back to its ___________ _______________ energy level (ground state) in the form of _________ ________________

33. Atomic Emission Spectrum (hydrogen) Each line in the spectrum results from a different ____________ ____________

34. Emission Spectrum: Iron (more e-) Carbon (less e-) Continuous Spectrum

35. Valence Electrons Electrons in the ________ energy level Electrons used to form ________ _______ Group# of Valence Electrons 1A (1) 2A (2) 3A (13) 4A (14) 5A (15) 6A (16) 7A (17) 8A (18)

36. Octet Rule In order to become most _______, all atoms need 8 valence electrons in the outermost energy level. ______ ______ already have 8 valence electrons which is why they are _______. Other elements _____ or _____ electrons by forming chemical bonds in order to have 8 ________ _______ in the outermost energy level.

37. Oxidation Numbers _____ generally ____ electrons to become more stable. –______ form ______ ions (charged atoms) _________ generally _____ electrons to become more stable. –_________ form _______ ions (charged atoms) GroupOxidation # 1A (1) 2A (2) 3A (13) 4A (14) 5A (15) 6A (16) 7A (17) 8A (18)