Nt1310 Unit 1 Lab 1
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I noticed that there is a relationship between the ionic radius and the atomic number of the representative elements in Group 1A. The higher the atomic number, the bigger the ionic radius is. So, while hydrogen has an atomic number of 1 and Francium has an atomic number of 87, it is safe to assume that FR has a higher ionic radius. This is true; the ionic radius for Hydrogen is 0.012, and for Francium, it is 0.194. The electrons that are gained or lost effect the ionic radius. If there is a positive charge, it would decrease the radius because that loses an electron. Whereas, if you had a negative charge, it would increase the radius because now there's an extra electron. I noticed that there's a relationship between the first ionization
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Lab 7: Moon Phases was designed to measure the relative position of the Sun and Moon over the course of one phase cycle (i.e. one month, 29.5 days) The idea for Lab 7: Moon Phases was to examine how the illumination of the moon by the Sun produces the different phase cycles we see as the Moon rotates around Earth and as the Earth rotates around the Sun. The observations of the Moon were taken on four different days in the month of February to March capturing four different Moon Phases.
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Parrish, We have a green light. One additional requirement, is that risk assessment team works with MAT to complete the following: 1) Work in tandem with Fred to "develop a criteria / written documentation to assess Wi-Fi access points (WAP) devices so when the risk assessors go out to perform their assessments that validation understands what to ask for and how to validate these devices for CS security to include "best practice" mitigation hardening for these devices. 2) Find out where all these Wi-Fi WAPs are included in the packages. Our database could be of use to them. (E.g. FARs comes to my mind as I know they use WAP) In additional, have them find out who else uses WAPs?
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Information Assurance Lab5: Introduction to Metasploit on Kali Linux Anti-Black Hats 1) Booting Kali Linux and starting Metasploit: 1d.) Why is it usually a bad idea to operate in the Linux environment as root? If you are unfamiliar with the concept of the root user, do a quick google search Answer: Root User: In Unix-like computer OSes, root is the conventional name of the user who has all rights or permissions (to all files and programs) in all modes (single- or multi-user. The root user can do many things an ordinary user cannot, such as changing the ownership of files and binding to network ports numbered below 1024.
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$A$ is a set of conditions $C_{i,L_j},{i,j}inmathbb{N}$ at the same hierarchical level $L_j$. Only one condition $Cin A$ can be extit{true} at the same time and no state transition without being specified by a condition is possible. If condition $C_{i,L_j}$ is not extit{true} any more (due to the proceeding of the assembly operation), there is a fallback to state $S_{j,L_i}$ and all conditions are evaluated to determine the current substate. An exemplary decomposition tree containing different hierarchical levels, multiple states per level and conditions for state transition is given by Fig.~
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1. Traffic control: As the data communication is the most energy-consuming part of the wireless sensor networks by decreasing the amount of traffic, energy can be saved. To distribute traffic effectively from a central node to other nodes, investigations are still needed in the network. 2. Preserve the traffic load balancing:
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Event 1. At point A corner of 74th St and Madison Avenue a LTB Mechanical Inc. employee parks his Van and seems very happy ( my personal comments S.H.) after find parking because of busy traffic in city. The driver goes to the nearby muni meter and inserts his credit card and he presses couple of buttons but was unable to buy the time card. He goes to the opposite corner and disappears.
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As a child we sung, “ Somewhere in the ancient, mystic trinity. You get three as a magic number. The past and the present and the future. Give you three as a magic number.”
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4.1 SEX-Dose sex differ will have influence on student’s score? From the histogram graphs above, we can confirm that mean in four subjects are trend to normally distributed. To test whether the mean for reading, writing, math and science is the same for males and females, an independent samples t-test tool is suitable because it can compare the means of a normally distributed interval dependent variable for two independent groups. H0: Females have no significant difference and high mean score than males in reading score H1:
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1. What were your results for the test? Were these results surprising to you? Why or why not? a.
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1a. Sodium has a larger radius than lithium because it has a higher principle quantum number and it’s electrons occupy more subshells. Because sodium and lithium are in the same group they both have 1 valence electron, but sodium has its outermost electron at n=3, and lithium’s outermost electron is at n=2, so sodium will have a larger radius despite effective nuclear charge. 1b. Magnesium has a smaller radius than sodium because it’s valence electrons have a stronger net attraction to the nucleus.
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Typically atomic radius increases as the elements go down a family. As the elements go down a family, they generally have an increasing number of energy levels or shells which results in an increased distance from the nucleus which makes the atom larger. Since the energy level is increasing, the screening level also increases. This means that the electrons are blocked and are held more loosely than other electrons closer to the nucleus. This causes the atom to be larger.
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The atomic radius cannot be measured directly because the electron cloud does not have a definite boundary. So, one way to measure the size of an atom is by calculating the bond radius, which is half the distance between the nuclei of two bonded atoms. Electron shielding (down a group, not across a period), effective nuclear charge, and the energy level that the outermost electrons occupy plays an major role in determining the atomic radius. On the periodic table, the atomic radius increases down a group because the energy level of the atom down the group increases from top to bottom causing the electrons to have more energy. The effective nuclear charge remain constant down a group because of electron shielding prevents the valence electrons
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On the right-hand side of the periodic table from the zigzag line, group 6 and group 7, like oxygen and chlorine, have outer shells which are nearly full. They're gain that extra one or two electrons to fill the shell up. When this happen, they become ions. The most atoms join together to create ions are group 1&2 and 6&7.
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Unit 3: Formation of ionic and metallic bonds Key unit competence: Describe how properties of ionic compounds and metals are related to the nature of their bonding 3.1. Introduction Activity 3.1 Look at the pictures above and answer the following questions. Record your answers and discuss them in your groups.
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6(c) The answers would not change because the bond angles between Cl-C-Cl and H-C-C do not affect the angle of rotation. 7(a) There are seven fluorine environments. 7(b)
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