2. 1 The Physical Setting Chemistry Jerry Deutsch

3. 2 New York State Education Department Core Curriculum http://www.emsc.nysed.gov/ciai/mst/pub/chemist.pdf

4. 3 I. Atomic Concepts

5. J Deutsch 2003 4 The modern model of the atom has evolved over a long period of time through the work of many scientists. (3.1a)  Democritus – matter is made up of particles called atoms  Dalton – atoms of the same element are alike – solid indivisible spheres  Thomson – discovers electrons – plum pudding model  Rutherford – gold foil experiment – discovers heavy, + charge nucleus – mostly empty space  Bohr – orbital model of electrons

6. J Deutsch 2003 5 Regents Question: 08/02 #1 Subatomic particles can usually pass undeflected through an atom because the volume of an atom is composed of (1) an uncharged nucleus (2) largely empty space (3) neutrons (4) protons

7. J Deutsch 2003 6 Regents Question: 01/03 #62-64 One model of the atom states that atoms are tiny particles composed of a uniform mixture of positive and negative charges. Scientists conducted an experiment where alpha particles were aimed at a thin layer of gold atoms. Most of the alpha particles passed directly through the gold atoms. A few alpha particles were deflected from their straight-line paths. An illustration of the experiment is shown below.

8. J Deutsch 2003 7 Regents Question cont’d Most of the alpha particles passed directly through the gold atoms undisturbed. What does this evidence suggest about the structure of the gold atoms? A few of the alpha particles were deflected. What does this evidence suggest about the structure of the gold atoms? How should the original model be revised based on the results of this experiment? Most of the atom is empty space. There is central + charge. The nucleus is +. The atom is not a uniform mixture of + and - charge. Positive charge is located in a heavy central mass.

9. J Deutsch 2003 8 Regents Question: 06/03 #67 John Dalton was an English scientist who proposed that atoms were hard, indivisible spheres. In the modern model, the atom has a different internal structure. Identify one experiment that led scientists to develop the modern model of the atom. Rutherford’s gold foil experiment

10. J Deutsch 2003 9 Regents Question cont’d John Dalton was an English scientist who proposed that atoms were hard, indivisible spheres. In the modern model, the atom has a different internal structure. Describe this experiment. State one conclusion about the internal structure of the atom, based on this experiment. Most of the atom is empty space. Rutherford’s shot alpha particles a piece of gold foil. Most of the alpha particles went through, some were deflected and some were reflected.

11. J Deutsch 2003 10 Each atom has a nucleus, with an overall positive charge, surrounded by one or more negatively charged electrons. (3.1b)

12. J Deutsch 2003 11 Subatomic particles contained in the nucleus include protons and neutrons. (3.1c)  Particles in the nucleus (protons and neutrons) are called nucleons  The mass of the atoms is concentrated in the nucleus  Electrons are not found in the nucleus, they orbit the nucleus.  The net charge of the nucleus is positive (+)

13. J Deutsch 2003 12 The proton is positively charged, and the neutron has no charge. The electron is negatively charged. (3.1d) Charge Mass

14. J Deutsch 2003 13 Regents Question: 01/03 #1 Which statement best describes electrons? (1)They are positive subatomic particles and are found in the nucleus. (2)They are positive subatomic particles and are found surrounding the nucleus. (3)They are negative subatomic particles and are found in the nucleus. (4)They are negative subatomic particles and are found surrounding the nucleus.

15. J Deutsch 2003 14 Regents Question: 06/02 #58-60 In the modern model of the atom, each atom is composed of three major subatomic (or fundamental) particles. Name the subatomic particles contained in the nucleus of the atom. State the charge associated with each type of subatomic particle contained in the nucleus of the atom. What is the net charge of the nucleus? Proton and neutron Proton is positive and the neutron is neutral Positive

16. J Deutsch 2003 15 Regents Question: 06/03 #2 Which subatomic particle has no charge? (1) alpha particle (2) beta particle (3) Neutron (4) electron

17. J Deutsch 2003 16 Protons and electrons have equal but opposite charges. The number of protons equals the number of electrons in an atom. (3.1e) # of protons = # of electrons Therefore, atoms are electrically neutral.

18. J Deutsch 2003 17 The mass of each proton and each neutron is approximately equal to one atomic mass unit. An electron is much less massive than a proton or a neutron. (3.1f) Charge Mass

19. J Deutsch 2003 18 The atomic number for an element cannot change but its mass number can.  Atomic Number –The number of protons in the nucleus of an atom –Determines which element  Mass Number –The number of nucleons (protons + neutrons) –If you don’t know the mass number you can round off the atomic mass for that element  # neutrons = mass # - atomic #

20. J Deutsch 2003 19 Regents Question: 06/02 #33 The number of neutrons in the nucleus of an atom can be determined by (1)Adding the atomic number to the mass number (2)Subtracting the atomic number from the mass number (3)Adding the mass number to the atomic mass (4)Subtracting the mass number from the atomic number

21. J Deutsch 2003 20 Regents Question: 06/03 #1 The atomic number of an atom is always equal to the number of its (1) protons, only (2) neutrons, only (3) protons plus neutrons (4) protons plus electrons

22. J Deutsch 2003 21 Regents Question: 08/02 #4 What is the total number of protons in the nucleus of an atom of potassium-42? (1) 15 (2) 19 (3) 39 (4) 42 The mass number (42) is not necessary to find the number of protons.

23. J Deutsch 2003 22 Regents Question: 06/03 #36 The nucleus of an atom of K-42 contains (1) 19 protons and 23 neutrons (2) 19 protons and 42 neutrons (3) 20 protons and 19 neutrons (4) 23 protons and 19 neutrons

24. J Deutsch 2003 23 In the wave-mechanical model (electron cloud model), the electrons are in orbitals, which are defined as the regions of the most probable electron location (ground state). (3.1h) An orbital is the area of highest probability of finding an electron.

25. J Deutsch 2003 24 Regents Question: 06/03 # 5 The region that is the most probable location of an electron in an atom is (1) the nucleus (2) an orbital (3) the excited state (4) an ion

26. J Deutsch 2003 25 Regents Question: 06/02 #2 The modern model of the atom shows that electrons are (1)orbiting the nucleus in fixed paths (2)found in regions called orbitals (3)combined with neutrons in the nucleus (4)located in a solid sphere covering the nucleus

27. J Deutsch 2003 26 Each electron in an atom has its own distinct amount of energy. (3.1i) When electrons are in their lowest energy state, it is called the ground state The ground state for Na is 2-8-1

28. J Deutsch 2003 27 The maximum number of electrons in a principal energy level (shell) is 2n 2. Energy level (n) Maximum number of electrons (2n 2 ) 12 28 318 432

29. J Deutsch 2003 28 Electron Configuration tells us how many electrons in each principal energy level (shell).  Atomic Number = 7  Mass Number = 14  7 protons  7 neutrons  7 electrons  Electron configuration: 2-5

30. J Deutsch 2003 29 The electron configuration for the ground state of an atom is given on the Periodic Table of the Elements. Electron Configuration

31. J Deutsch 2003 30 Regents Question: 06/02 #1 What is the electron configuration of a sulfur atom in the ground state? (1)2-4 (2)2-6 (3)2-8-4 (4)2-8-6 Look at the Periodic Table of the Elements If you do not know the symbol for sulfur, check Table S

32. J Deutsch 2003 31 When an electron in an atom gains a specific amount of energy, the electron is at a higher energy state (excited state). (3.1j) Possible excited states for Na are: 2-7-2 1-8-2

33. J Deutsch 2003 32 When an electron returns from a higher energy state to a lower energy state, a specific amount of energy is emitted. This emitted energy can be used to identify an element. (3.1k) Emission Spectrum

34. J Deutsch 2003 33 Regents Question: 01/03 # 2 During a flame test, ions of a specific metal are heated in the flam of a gas burner. A characteristic color of light was emitted by these ions in the flame when the electrons (1)Gain energy as they return to lower energy levels (2)Gain energy as they move to higher energy levels (3)Emit energy as they return to lower energy levels (4)Emit energy as they move to higher energy levels

35. J Deutsch 2003 34 Regents Question: 06/03 # 3 When the electrons of an excited atom return to a lower energy state, the energy emitted can result in the production of (1)alpha particles (2) Isotopes (3) protons (4) spectra

36. J Deutsch 2003 35 Regents Question: 06/03 #51-52 Base your answers to the next two questions on the electron configuration table shown below. What is the total number of valence electrons in an atom of electron configuration X? Which electron configuration represents the excited state of a calcium atom? Element Electron Configuration X 2 –8 –8 –2 Y 2 –8 –7 –3 Z 2 –8 –8 2 2-8-7-3

37. J Deutsch 2003 36 The outermost electrons in an atom are called the valence electrons. In general, the number of valence electrons affects the chemical properties of an element. (3.1l) The ground state for Na is 2-8-1 The valence shell is the third shell. The valence shell contains 1 electron.

38. J Deutsch 2003 37 Regents Question: 08/02 #2 What is the total number of electrons in the valence shell of an atom of aluminum in the ground state? (1)8 (2)2 (3)3 (4) 10

39. J Deutsch 2003 38 Regents Question: 06/02 #31 In which shell are the valence electrons of the elements in Period 2 found? (1)1 (2)2 (3)3 (4)4

40. J Deutsch 2003 39 Atoms of an element that contain the same number of protons but a different number of neutrons are called isotopes of that element. (3.1m) Isotopes of Hydrogen 1 H – protium1 proton0 neutron 2 H – deuterium1 proton1 neutron 3 H – tritium1 proton2 neutrons

41. J Deutsch 2003 40 Regents Question: 01/03 #9 An atom of carbon-12 and an atom of carbon-14 differ in (1)Atomic number (2)Atomic mass (3)Nuclear charge (4)Number of electrons Carbon-12 and carbon-14 are isotopes.

42. J Deutsch 2003 41 Regents Question: 06/02 #4 All the isotopes of a given atom have (1)the same mass number and same atomic number (2)the same mass number but different atomic numbers (3)different mass numbers but the same atomic number (4)different mass numbers and different atomic number

43. J Deutsch 2003 42 Regents Question: 06/02 #9 Atoms of the same element that have different numbers of neutrons are classified as (1)Charged atoms (2)Charged nuclei (3)Isomers (4)Isotopes

44. J Deutsch 2003 43 The average atomic mass of an element is the weighted average of the masses of its naturally occurring isotopes. (3.1n) IsotopeMassAbundanceCalculation 12 C1298.89%12 x.9889 = 11.87 13 C131.108%13 x 0.01108 = 0.1440 Atomic Mass (weighted average) 12.01 amu

45. J Deutsch 2003 44 Regents Question: 06/03 # 4 The atomic mass of an element is calculated using the (1) atomic number and the ratios of its naturally occurring isotopes (2) atomic number and the half-lives of each of its isotopes (3) masses and the ratios of its naturally occurring isotopes (4) masses and the half-lives of each of its isotopes

46. J Deutsch 2003 45 Regents Question: 01/03 #36 Hydrogen has three isotopes with mass numbers of 1, 2, and 3 and has an average atomic mass of 1.00794 amu. This information indicates that (1)Equal number of each isotope are present (2)More isotopes have an atomic mass of 2 or 3 than 1 (3)More isotopes have an atomic mass of 1 rather than 2 of 3 (4)Isotopes have only an atomic mass of 1

47. J Deutsch 2003 46 Regents Question: 01/03 #3 In which list are the elements arranged in order of increasing atomic mass? (1)Cl, K, Ar (2)Fe, Co, Ni (3)Te, I Xe (4)Ne, F, Na Look for the masses on the periodic table of the elements.