Nt1310 Unit 1 Atomic Theory

1-1: Insert the chemical symbol in the answer blank for each of the following elements.

Concept 2.1 Matter consists of chemical elements in pure form and in combinations called compounds

The students created a macroscopic, three-dimensional (3D) model of several properties of the periodic table. They explained in their own words the following terms: atomic radii, ionic radii, first ionization energy, and electronegativity. Lastly, they identified, described, and explained the patterns observed in the 3D periodic tables for the following element properties: atomic radii, ionic radii, first ionization energy, and electronegativity.

5) List the three common states of matter in order of highest potential to lowest.

1. Arrange the following molecules from least to most specific with respect to the original nucleotide sequence: RNA, DNA, Amino Acid, Protein

E. have bonds with an overall positive charge. Correct See Section 2.2: How Do Atoms Bond to Form Molecules? Points Earned: 1/1 Correct Answer: A Your Response: A 2.

F 7. H 8. C 9. E 10. J 11.

a. atoms lose electrons if they have just one or two electrons in their valence shells; they gain electrons if they need just one or two electrons to complete the valence shell as in K+CL- __Ionic bonds_

5) List the three common states of matter in order of highest potential to lowest.

To be a stable atom, most elements need eight electrons in their outmost shell, also referred to as the octet rule (OpenStax 2015). When atoms are in their ground state, the electrons are in the lowest energy level and closest to the nucleus. The levels are represented by the letter n. For the lowest energy level, n is equal to 1 and as the electron increases in energy level the n increases by whole number, because electrons cannot exist between the energy levels. When an electron gains energy, it is in its excided state.

Mulliken atomic charge

The purpose of this lab was to determine the atomic structure of small molecules and ions which we did by drawing Lewis Dot Structures, drawing molecular geometries, and using the VSEPR model on a computer. The VSEPR Theory states that molecular geometries of molecules can be predicted through their number of electron pairs on the central atom because these electrons will repulse each other as much as they can while still being bound to the central atom. The Lewis Dot Structures and the molecular geometries that we were asked to draw were in order for us to have background knowledge of how each molecule was shaped before we had to make them on the computer.

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.

Fig. 4 shows that in the valence band near the Fermi level, the spin-up

A atom of one element is divided to create two small atom of different elements