Human Resource performance evaluation systems in organization

The performance evaluation system of Maple leaf shoes is so ineffective hence affecting the overall performance of the company. Performance evaluation system must be one which creates motivational opportunities to employees. What happens in Maple leaf shoes is discouraging to workers.Advertising We will write a custom case study sample on Human Resource: performance evaluation systems in organization specifically for you for only $16.05 $11/page Learn More More than 75% of company’s employee had negative feelings about the system. This means that many workers are not satisfied with the manner in which they get assessed. Supervisors fail to meet their obligations by not conducting the assessment process as expected. It is said that some supervisors fill in appraisal forms in three minutes. In fact, there is no way an employee can be assessed in three minutes. This shows negligence among supervisors in doing their work. The company’s manageme nt also has played a role in poor assessment. This is because actions are not taken to reflect employees’ performance. Since no promotions are effected based on the assessment reports, supervisors consider the assessment as a useless exercise. As a result, they fill in the assessment forms just to amuse their bosses but not for the best of the company. I would recommend that supervisors receive thorough training in order to understand the essence of carrying out employee assessment. Then management should take actions depending on the reports drafted from the appraisal forms. For example, performers should be rewarded by either promotion or monetary gifts. Those not performing well should also be involved in discussing their performance, and this can help identify their areas of weakness. Once the weak points are identified management can provide possible solutions hence increasing employees’ performance. The system of assessing employee performance should be restructu red to ensure that employees accept the outcomes. When these changes are implemented, employees can enjoy healthy working relationships hence giving their best to the company. For the case of Canadian Pacific and International Bank, a 360 degrees performance evaluation system has been faced with opposition from some section of managers. If I were in Mary Keddy’s position, I would work with the managers supporting the system to pull the rest into supporting it. The first step is to engage middle managers in a discussion regarding the new performance system. Make them understand the benefits of successful 360 degrees performance evaluation systems. The managers should be allowed to air their fears about the new system and then all issues discussed. She should make sure that all fears raised are satisfactorily addresses and then together with the managers they should lay down strategies for implementation.Advertising Looking for case study on business economics? Let's see if we can help you! Get your first paper with 15% OFF Learn More The next step should be training employees on how to evaluate their seniors and their fellow colleagues in the right direction. This ensures that backstabbing is not given a chance in the process of evaluation hence concentrating on areas suited for the best of the company. Since this system involves everybody in the company evaluating their colleagues, managers and their juniors, the evaluation forms should be guided by the human resource representatives. For example, questionnaires meant for evaluating managers should contain areas which concerns performance. This helps control circumstances where workers may be bitter with their supervisors and would like to express all their feelings on the evaluation form. After everyone is convinced about the introduction of the new evaluation plan, Mary can proceed and introduce the evaluation system in the company. She should give details of when assessment will be don e and make sure everybody takes part in the process. This case study on Human Resource: performance evaluation systems in organization was written and submitted by user Rumiko Fujikawa to help you with your own studies. You are free to use it for research and reference purposes in order to write your own paper; however, you must cite it accordingly. You can donate your paper here.

Ionization Energy of the Elements

Ionization Energy of the Elements The ionization energy, or ionization potential, is the energy required to completely remove an electron from a gaseous atom or ion. The closer and more tightly bound an electron is to the nucleus, the more difficult it will be to remove, and the higher its ionization energy will be. Key Takeaways: Ionization Energy Ionization energy is the amount of energy needed to completely remove an electron from a gaseous atom.Generally, the first ionization energy is lower than that required to remove subsequent electrons. There are exceptions.Ionization energy exhibits a trend on the periodic table. Ionization energy generally increases moving from left to right across a period or row and decreases moving top to bottom down an element group or column. Units for Ionization Energy Ionization energy is measured in electronvolts (eV). Sometimes the molar ionization energy is expressed, in J/mol. First vs Subsequent Ionization Energies The first ionization energy is the energy required to remove one electron from the parent atom. The second ionization energy is the energy required to remove a second valence electron from the univalent ion to form the divalent ion, and so on. Successive ionization energies increase. The second ionization energy is (almost) always greater than the first ionization energy. There are a couple of exceptions. The first ionization energy of boron is smaller than that of beryllium. The first ionization energy of oxygen is greater than that of nitrogen. The reason for the exceptions has to do with their electron configurations. In beryllium, the first electron comes from a 2s orbital, which can hold two electrons as is stable with one. In boron, the first electron is removed from a 2p orbital, which is stable when it holds three or six electrons. Both of the electrons removed to ionize oxygen and nitrogen come from the 2p orbital, but a nitrogen atom has three electrons in its p orbital (stable), while an oxygen atom has 4 electrons in the 2p orbital (less stable). Ionization Energy Trends in the Periodic Table Ionization energies increase moving from left to right across a period (decreasing atomic radius). Ionization energy decreases moving down a group (increasing atomic radius). Group I elements have low ionization energies because the loss of an electron forms a stable octet. It becomes harder to remove an electron as the atomic radius decreases because the electrons are generally closer to the nucleus, which is also more positively charged. The highest ionization energy value in a period is that of its noble gas. Terms Related to Ionization Energy The phrase ionization energy is used when discussing atoms or molecules in the gas phase. There are analogous terms for other systems. Work Function - The work function is the minimum energy needed to remove an electron from the surface of a solid. Electron Binding Energy - The electron binding energy is a more generic term for ionization energy of any chemical species. Its often used to compare energy values needed to remove electrons from neutral atoms, atomic ions, and polyatomic ions. Ionization Energy Versus Electron Affinity Another trend seen in the periodic table is electron affinity. Electron affinity is a measure of the energy released when a neutral atom in the gas phase gains an electron and forms a negatively charged ion (anion). While ionization energies may be measured with great precision, electron affinities are not as easy to measure. The trend to gain an electron increases moving from left to right across a period in the periodic table and decreases moving from top to bottom down an element group. The reasons electron affinity typically becomes smaller moving down the table is because each new period adds a new electron orbital. The valence electron spends more time further from the nucleus. Also, as you move down the periodic table, an atom has more electrons. Repulsion between the electrons makes it easier to remove an electron or harder to add one. Electron affinities are smaller values than ionization energies. This puts the trend in electron affinity moving across a period into perspective. Rather than a net release of energy when an electron is gain, a stable atom like helium actually requires energy to force ionization. A halogen, like fluorine, readily accepts another electron.