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Atoms-Molecules-Ions

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1 Atoms-Molecules-Ions
Dr. Ron Rusay © Copyright R.J. Rusay

2 Aspects of Matter Elements, Compounds, and Mixtures (Part 1)
Atomic Theory Today Elements: The Periodic Table Ions & Compounds Compounds: Introduction to Ionic Bonding Compounds: Formulas & Names (Part 2) Mixtures: Separation Techniques (Part 3) Atomic & Molar Masses (Part 4)

3 Modern History of the Atom
1909: Millikan determines charge and mass of e- : Rutherford & Bohr’s atom; The proton. 1927: Waves & Particles, Quantum Mechanics 1932: James Chadwick “discovers” the neutron © Copyright R.J. Rusay

4 CHEMISTRY of the Atom Ernest Rutherford (1871-1937)

5 Modern History of the Atom
1897: J.J. Thomson “discovers” the electron: Photo © The Nobel Foundation © Copyright R.J. Rusay

6 Milliken Oil Drop Experiment

7 (12.76 x 10 6), 12.76 million meters (megameters)
How does an atom relate to nanotechnology? Consider Powers of 10 (10 x) Plant Cell = meters wide (12.76 x 10 -6) (12.76 millionths of a meter) (12,760 nanometers!) Earth = 12,760,000 meters wide (12.76 x 10 6), million meters (megameters) Nano scale is regarded as < 1,000 nanometers ~1/50 the diameter of a human hair (anything less than a micron (10-6 m). Chemists typically think in views and images of < 1 nanometer (eg. bond lengths and atomic sizes).

8 1 Å = 10 picometers = 0.1 nanometers =
~ 0.1 nm Anders Jöns Ångström ( ) 1 Å = 10 picometers = 0.1 nanometers = 10-4 microns = 10-8 centimeters Nucleus = 1/10,000 of the atom 1 nm = 10 Å An atom vs. a nucleus ~10,000 x larger

9 Can we “see” and manipulate atoms using a microscope?
Yes, using atomic force microscopy (AFM) and a variety of instruments such as Scanning Transmission Electron Microscopes. TEAM 0.5: LBL’s Latest (2008) Transmission Electron Aberration-corrected Microscope Resolution: +/- 0.5 Å 1 nm = 10 Å An atom vs. a nucleus ~10,000 x larger

10 Atomic/molecular structures atom-by-atom
Building of a quantum “corral” with Fe atoms on Cu Xe atoms on Ni(110) STM images courtesy of Don Eigler, IBM, San Jose

11 Imaging: acetylene on Pd(111) at 28 K
H Molecular Image Tip cruising altitude ~700 pm Δz = 20 pm Why don’t we see the Pd atoms? Because the tip needs to be very close to image the Pd atoms and would knock the molecule away p orbital pz TIP H O + Surface atomic profile Tip cruising altitude ~500 pm Δz = 2 pm Calculated image (Philippe Sautet) If the tip was made as big as an airplane, it would be flying at 1 cm from the surface and waving up an down by 1 micrometer The STM image is a map of the pi-orbital of distorted acetylene 1 cm (± 1 μm) M. Salmeron (LBL)

12 Excitation of frustrated rotational modes in acetylene molecules on Pd(111) at T = 30 K
Tip e- ((( ) ( ))) M. Salmeron (LBL)

13 The particle is said to “hold” or “bond” atoms together in molecules.
CHEMISTRY of the Atom FUNDAMENTAL PARTICLES: Mass Charge Symbol Nucleus: PROTON amu H+, H, p 1.67 x kg NEUTRON amu n _________________________________________ ELECTRON very small e -  2000 x smaller than a proton or neutron The particle is said to “hold” or “bond” atoms together in molecules. © Copyright R.J. Rusay

14 Periodic Table Mendeleev’s Table 1868-1871
Mural at St.Petersburg University, Russia © Copyright R.J. Rusay

15

16 QUESTION The element found in the 6A family (or group 16) and period four can be toxic, a micronutrient, and found in compounds in dandruff shampoos. What is the symbol for that element? Sb As Se Te

17 Chemical Symbols & Historical Names
What is the symbol for gold and what was its original name?

18 QUESTION

19

20 QUESTION Of the following which would not be considered a metalloid?
Ge Sb Te Se As

21 Periodic Table Elements are classified by: properties & atomic number
metals, non-metals, metalloids Groups or Families (vertical) 1A = alkali metals 2A = alkaline earth metals 6A (16) = chalcogens 7A (17) = halogens 8A (18) = noble gases Periods (horizontal) numbers 1-7

22 QUESTION Select the correct statement relative to the modern periodic table. A) Tin is a transition element. B) Lead is a nonmetal. C) Antimony is a metalloid. D) Elements are arranged in order of increasing atomic mass. E) Sulfur is a halogen.

23 Group 1 and Group 2 Metals

24 Using the Periodic Table

25 Atoms, Molecules & Ions Atoms (neutral electrostatic charge: # protons = # electrons ) # Protons = Atomic Number Atomic Mass = # Protons + # of Neutrons Isotope: same atomic number but different atomic mass (different # of neutrons) © Copyright R.J. Rusay

26 QUESTION

27 Atoms, Molecules & Ions Isotopes vary in their relative natural abundance. Periodic Table’s atomic mass is a weighted average of all isotopic masses The mass of sodium, Na, element #11 is listed as amu. Which isotope is naturally present in the larger amount: the isotope with 12 neutrons or with 13 neutrons? (There is a small percentage of the isotope with 11 neutrons.) © Copyright R.J. Rusay

28 QUESTION Two stable isotopes of an element have isotopic masses of amu and amu. The atomic mass is Which isotope is more abundant? A) There is insufficient information to answer the question. B) There are equal amounts of each isotope. C) The isotope with a mass of amu is more abundant. D) The isotope with a mass of amu is more abundant. Correct Answer: D Question Number: 10

29 Atoms, Molecules & Ions Atomic Mass of Carbon:
What is the “weighted” atomic mass? © Copyright R.J. Rusay

30 QUESTION The two major isotopes of bromine are 79Br and 81Br.
Assume that the masses of the 79Br and 81Br isotopes are and amu, respectively. The weighted average atomic mass of bromine is amu. What are the relative % abundances of each isotope? % Abundance of 79Br % Abundance of 81Br 79.0% % 19.0% % 35.1% % 55.0% % Correct Answer: D Question Number: 12

31 Atoms, Molecules and Ions
Atomic Number = 6 (atom’s identity) Carbon Atomic Mass = 13 (isotope 13) 6 protons; # neutrons = neutral atom has 6 electrons © Copyright R.J. Rusay

32 QUESTION

33 K K 39 19 39 Atomic Symbols Mass number   Element Symbol
Atomic number  39 K Also written as 

34 Atoms, Molecules and Ions
Atomic Number = 12 (atom’s identity) Atomic Mass = 24 12 protons; # neutrons = neutral atom has 12 electrons Ion contains 10 electrons: symbol? 12 p e- = +2 © Copyright R.J. Rusay

35 Atoms, Molecules and Ions
Atomic Number = 17 (atom’s identity) Atomic Mass = ? # protons = ? ; # neutrons = ? neutral atom has ? electrons Ion contains 18 electrons: symbol? 17 p e- = -1 © Copyright R.J. Rusay

36 Ions Cation: A positive ion Mg2+, NH4+ Anion: A negative ion
Cl, SO42 Ionic Bonding: Force of attraction between oppositely charged ions.

37 QUESTION Calcium plays several critical roles in the functioning of human cells. However, this form of calcium is the ion made with 20 protons and 18 electrons. Therefore the ion would be… positive and called an anion. positive and called a cation. negative and called an anion. negative and called a cation.

38 QUESTION Of the following, which would NOT qualify as an isotope of 35Cl? 36Cl 35Cl– 37Cl– 37Cl

39 Worksheet: Atoms I (Lab Manual)

40 Which of these species has the highest number of electrons?
QUESTION Which of these species has the highest number of electrons? A) 20Ca B) 19K+ C) 16S2− D) 15P3−

41

42 QUESTION The ion 45Sc3+ has
A) 24 electrons, 21 protons and 24 neutrons B) 18 electrons, 21 protons and 24 neutrons C) 24 electrons, 24 protons and 21 neutrons D) 18 electrons, 24 protons and 21 neutrons

43 Polyatomic Ions

44 Molecules Neutrally Charged Eg. Salt: NaCl -> 1 Na+ and 1 Cl -
What is the proportion of ions for a compound formed from Mg ion and chlorine? Mg2+ and Cl 1 Mg2+ combines with 2 Cl

45

46 Ionic vs. Covalent

47 Ionic vs. Covalent Metals generally combine with non- metals to form ionic compounds. Electrons are “lost” by the metal and “gained” by the non-metal following the octet rule. Non-metals generally combine with non-metals to form covalent compounds where electrons are “shared”. Each pair of electrons ia a covalent bond. Eg. H2O Polyatomic ions have both covalent and ionic properties. Eg. hydroxide, OH-

48 QUESTION

49 C20 H26 N2 O (Ibogaine, not ionic)
Chemical Formulas Molecular Formula: Elements’ Symbols = atoms Subscripts = relative numbers of atoms How many atoms of each element are in the following componds? MgCl2 CCl4 NaOH (NH4 )2CO3 C20 H26 N2 O (Ibogaine, not ionic)

50 QUESTION

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