Nt1310 Unit 9 Lab Report

Q1. Illustrate an atom (using pen and paper – not a google image!). Label each part of the structure.

Mercury has 121 neutrons and 80 protons in its nucleus. It also has 6 electron shells with 2 electrons in the first shell, 8 electrons in the second shell, 18 electrons in shell 3, 32 electrons in the fourth shell, 18 electrons in the fifth shell and 2 in the sixth

The atoms of each element possess a unique electron configuration because of the fact that different elements have different numbers of electrons. The ground state electron configuration shows both the lowest and most stable position for each element. There are three basic rules used for determining the ground-state electron configurations.

Vanadium, pronounced veh-NAY-di-em, atomic symbol V, and atomic number associated with this transition metal is 23. The atomic weight of Vanadium is 50.942 grams per one mole. The electron configuration is 1S2 2S2 2P6 3S2 3P6 4S2 3D3 and the noble gas notation is [Ar] 4S2 3D3.

Lewis Structure shows how atoms in a covalent bond share electrons. Dots are used to show lone pairs of electrons, and lines symbolize bonds. This essay will explain how Lewis Structures are constructed.

The six electrons that are around the nucleus are very important. 2 of the 6 electrons are deep at the inner core and don’t have an effect on the interaction with other elements. The 4 electrons on the outermost layer are active. These

Electrons always fill orbitals with lower energy levels. The 4s sublevel is lower in energy than the 3d sublevel, so the 4s sublevel will get filled first.

Explain how an element’s group in the periodic table can be used to predict its outer shell electrons.

Just like the elements in its group, “Da” is an alkaline earth metal with similar properties as the others above it, and a +2 oxidation state as well. The complete electron configuration will be as

Each shell has a maximum number of electrons it can contain, with the first shell containing up to 2, the second shell containing up to 8 and the third shell containing up to 18. However, each electron shell follows the octet rule and generally only contains a maximum of 8 electrons. The electrons that are located in an atom’s outermost shell are called valence electrons. Atoms are arranged on the periodic table with the horizontal rows, called periods corresponding to the number of electron shells in an atom and the vertical columns, called groups corresponding to the number of valence electrons in an atom. The reactivity of an atom and its tendency to interact and form bonds with other atoms is determined by the number and distribution of the electrons. This arrangement allows these properties to be predicted easily.

(-- removed HTML --) (-- removed HTML --) 3 (-- removed HTML --) (-- removed HTML --) In this case, electrons as free particles form a partially filled conduction band. However, the permittivity of a large group of metals is affected by interband transitions of valence band electrons in addition to conduction band electrons in the optical spectrum. (-- removed HTML --)

6. Compare the meanings of atomic number, mass number, ion, and molecule. (p. 29) ANSWER:

27. Draw the Lewis structure for H2SeO4. If the valence shells are filled to the usual limit (maximum of 8), what is the formal charge on the Se?

3         single state “cube”: Vsingle state              a  b  c   V  4 “fermi-sphere”: Vfermi-sphere    k 3f    3  

2 (9.0) 1. a) Write a Lewis structure for each of the following compounds showing any unshared electron pairs. b) Calculate the formal charge on each atom other than hydrogen. Be sure to show your calculations. a) CH3OH2 EC(c) = 1/2(8) = 4 FC(c) = 4- 4 = 0