Essay on Atoms

For the lesson observed the objectives was to explain the trends of the periodic table based on the elements’ valence electrons and atomic numbers. Additionally, students were responsible for applying their previous knowledge in calculating subatomic particles to review the Bohr Models and discus the relationship among families in the periodic table. Students will use the information from today’s lesson to make future judgments on reactivity and bonding created during chemical reactions in the next unit. Lastly, students were to connect the information on elemental properties to previous experiences with their health, commercial products, and everyday life.

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.

An ionic bond is a bond that results from the attraction between oppositely charges ions; one atom "gives" another atom an electron. Combinations of metals and nonmetals typically form ionic bonds. A covalent bond is a bond that results from

A covalent bond is a bond that occurs when atoms in a molecule share a pair of electrons. For example, “the atoms in sugar do not form ions; instead, they are held together because of shared electrons.”

Vocabulary: atomic number, atomic radius, Aufbau principle, chemical family, diagonal rule, electron configuration, Hund’s rule, orbital, Pauli exclusion principle, period, shell, spin, subshell

As a result of the water molecule bond, each (hydrogen; oxygen) has a slightly negative charge and each (hydrogen; oxygen) has a slightly positive charge.

Heisenberg realized that the uncertainty relations had profound implications. Heisenberg set himself to the task of finding the new quantum mechanics to explain what his theories observed. He relied on what can be observed, namely the light emitted and absorbed by the atoms. By July 1925, Heisenberg wrote his answer in a paper. The basic idea of Heisenberg's paper was to get rid of the orbits in atoms and to arrive at new mechanical equations. Heisenberg’s approached focused mainly on the particle nature of electrons. The mathematics Heisenberg used were tables commonly used for multiplication of arrays of numbers-mathematical objects known as matrices. Using the mathematics of matrices, scientists had at last a new mechanics for calculating the quantum behavior of particles. Heisenberg, and others showed that the new quantum mechanics could account for many of the properties of atoms and atomic events.

B) Covalent bonds bind the atoms to each other in an organic molecule (Open Learning Initiative, 2015, pg.63).

35. Polyatomic ions (Table E) are groups of atoms, covalently bonded together, with an overall charge.

The main point of lecture was to continue discussing about the light spectra and atoms. Specifically, we used the equations and calculated a photon of light’s energy at a certain wavelength. Also, we discussed the light spectrum and how particular wavelengths of light are absorbed by matter.

Use VSEPR theory to predict the shape of a molecule based on its Lewis structure.

7. The more-electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion.

The 13C NMR Spectrum reveals the chemical environments of the C-H bonds. In this experiment, the carbons were assigned a number, from C1 to C4. C4 appeared the most downfield because it was the most deshielded because it is double bonded directly to an O and thus the O pulls the most on electron density. C3 is the most upfield because it is not bonded directly to any electron withdrawing groups or electronegative atom. C1 is the second most deshielded because this carbon is involved in a double bond which draws electron density. C2 appears second most upfield because this carbon is single bonded to an oxygen, but it is not as electron pulling as C4 or C1 that is double

The studies of chemistry and physics have shaped understanding of the world today. In fact, they have altered the mindset and reasoning of society, leading to an age in which discoveries are consistently being sought after and achieved. However, it must be noted that the origin for the basis of understanding used today in fields such as chemistry derived almost entirely from the scientists of the 1800’s. In this thorough and precise essay, the incubator for some of the world’s most innovative researchers and pioneers in chemistry and physics will be discussed – the Cavendish Laboratory.

At almost the same point in time, Kekule in Germany, and Couper of Scotland suggested that atoms in molecules are fused together by bonds. Their theory was that every atom is distinguished by having the same number of bond availability or valence number, where ever that particular atom appears in any compound. The main notability of organic compounds is having strong carbon to carbon bonds. This was recognized in the theory, and was used to help understand large molecules, possessing many bonded carbon atoms. Carbon is the cement that holds their molecules together. So far, this theory has gone through rigorous testing, and has not been proven inadequate to this day, as of now it is a law.