An octet rule is a chemical rule that indicates that the atoms of the main group elements have a tendency to combine in a manner that makes every atom to possess eight electrons in its valence shell. This combination gives atom to have an electronic configuration which is the same as the electronic configuration of noble gasses. The octet rule applies to oxygen, nitrogen, halogen gas and carbon. Besides, it is appropriate for metals like magnesium and sodium (Califano, 2012). 2
Aufbau rule asserts that theoretically, electrons that orbit more or one atom often fill the lowest available energy levels before filling the higher energy levels, for instance, if the available energy levels are 1s and 2s, 1s orbital will be filled first before filling
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Atom is referred to as the smallest and unnoticeable unit of matter. However, ions are atoms in which the number of protons and electrons are not the same. Therefore, ions can either be negatively and positively charged. Atom is made up of neutrons, protons, and electrons. The neutrons and protons make the nucleus of an atom while the electrons surround atom’s nucleus. Atom is electrically neutral because the number of electrons and protons are the same. Neutral Magnesium (Mg) is an atom, and it has 12 electrons and 12 electrons giving it a mass number of 24g/mole. Magnesium easily loses two electrons in its valence shell to be positively charged (cation), the number of protons are greater than the number of electrons in this case. Neutral oxygen (O) with eight electrons and eight protons is an atom. Oxygen atom easily acquire two extra electrons to make it valance shell complete and to become negatively charged; in this case, the number of electrons is more than the number of protons hence it is known anion (Smirnov, 2003). When an atom loses the electrons in their valence shell to become a cation, its atomic radius is always larger than it ionic radius. When an atom attracts electrons to its valence shell to become anion its atomic radius and ionic radius are the same (Housecroft, and Sharpe
Just as the title of the chapter suggests, the main focus of Chapter 11 is how elements found on the Periodic Table are not always what they appear. Kean begins this chapter with describing how elements can be unpredictable in some conditions, and uses example from the past to...
Oxygen is the first element on the Oxygen group. That is why the name of the group is named the Oxygen group. It has eight electrons total. It has six in its outer electron cloud. According to the octet rule, the oxygen will want to gain two more electrons to fill its outer shell with eight. Oxygen is also one of th...
Ionic compounds are normally a combination of a metal, along with one or more non-metals. If you recognize the two ions, you have the name of the compound. For example, the familiar calcium ion, Ca2+ must combine with two iodides, I–, to afford calcium iodide, CaI2. For ionic compounds this means that the formula unit must have an equal number of positive and negative charges because ionic
Lithium has an atomic number of 3, and an atomic weight of 6.94. In general, lithium is more stable than hydrogen, and slightly less stable than nitrogen, carbon, and oxygen. When looking at chemical ion properties, it is useful to consider three main characteristics: the size, or radius, of the ion, the charge, and the ion's electron affinity. Lithium has a similar charge to radius ratio to that of magnesium, which is in group IIA of the periodic table, and so chemists say that the two elements are "chemically similar.
Atoms are electrically neutral; the electrons that bear the negative charge are equal in number to the protons in the nucleus
In 1907, Einstein used Planck’s hypothesis of quantization to explain why the temperature of a solid changed by different amounts if you put the same amount of heat into the material. Since the early 1800’s, the science of spectroscopy had shown that different elements emit and absorb specific colors of light called “spectral lines.” In 1888, Johannes Rydberg derived an equation that described the spectral lines emitted by hydrogen, though nobody could explain why the equation worked. This changed in 1913 when Danish physicist Niel Bohr applied Planck’s hypothesis of quantization to Ernest Rutherford’s 1911 “planetary” model of the atom, which affirmed that electrons orbited the nucleus the same way that planets orbit the sun. Bohr offered an explanation for why electrical attraction does not make the electrons spiral into the nucleus. He said that electrons in atoms can change their energy only by absorbing or emitting quanta. When an electron absorbs a quantum it moves quickly to orbit farther from nucleus. When an electron emits a quantum the electron jumps to a closer
The Pauli exclusion principle is defined by Dr. Steven S. Zumdahl, "In a given atom no two electrons can have the same set of four quantum numbers." Due to this principle, only two electrons can inhabit a single energy level. The electrons that share the same energy level have opposite intrinsic angular momentums which is more commonly known as "spin". To determine the direction of the spin the angular momentum vector is analyzed.
An atom, by definition, is the smallest part of any substance. The atom has three main components that make it up: protons, neutrons, and electrons. The protons and neutrons are within the nucleus in the center of the atom. The electrons revolve around the nucleus in many orbitals. These orbitals consist of many different shapes, including circular, spiral, and many others. Protons are positively charged and electrons are negatively charged. Protons and electrons both have charge of equal magnitude (i.e. 1.602x10-19 coulombs). Neutrons have a neutral charge, and they, along with protons, are the majority of mass in an atom. Electron mass, though, is negligible. When an atom has a neutral charge, it is stable.
Out of all cations (positive ions) found in the human body, Magnesium is the fourth most abundant. Over half, usually between 50 and 60% is found in our skeletons. The other 40 to 50% is found evenly
While all atoms of the same element have the same number of protons, it is possible for atoms of one element to have different numbers of neutrons. Atoms of the same element with different numbers of neutrons are called isotopes . For example, all atoms of the element carbon have 6 protons, but while most carbon atoms have 6 neutrons, some have 7 or 8. Isotopes are named by giving the name of the element followed by the sum of the neutrons and protons in the isotope's nucl...
be Higher, as there are more atoms found in a smaller space. This leaves less, and smaller, gaps for the electrons to flow through. Because of the lack of space, we would expect there to be more collisions between. the atoms and electrons. Preliminary results:.
Isotopes: Atoms of the same element (same atomic number) but with differing numbers of neutrons, different mass numbers.
To start off, learning the Bohr-Rutherford diagrams in grade nine was a very big confusion for me. I had never fully understood how many shells should go around the nucleus nor did I know how to do the many calculations. As I progressed into grade ten, the teachings became easier. The review shows an example such as in the the bohr diagram, a nucleus is in the center, which is a little circle, and following that there are shells surrounding it containing electrons. Each ring can only hold a certain amount of electrons, and so the first shell around the nucleus can hold a maximum of 2 electrons, the next shell is able to hold a maximum of 8 electro...
This law states that, “when elements are arranged in order of increasing atomic number, there is a periodic repetition of their chemical and physical properties” (textbook). From that, the modern periodic table was born; “each new horizontal row of the table corresponds to the beginning of a new period because a new principal energy level is being filled with electrons” (textbook).
From these properties of bonds we will see that there are two fundamental types of bonds--covalent and ionic. Covalent bonding represents a situation of about equal sharing of the electrons between nuclei in the bond. Covalent bonds are formed between atoms of approximately equal electronegativity. Because each atom has near equal pull for the electrons in the bond, the electrons are not completely transferred from one atom to another. When the difference in electronegativity between the two atoms in a bond is large, the more electronegative atom can strip an electron off of the less electronegative one to form a negatively charged anion and a positively charged cation. The two ions are held together in an ionic bond because the oppositely charged ions attract each other as described by Coulomb's Law.