Organizational Behavior the Family, College Class, and Organization

Organizational Behavior the Family, College Class, and Organization The organizational Behavior The family is the society’s key organization. It is extremely imperative that the family engages in family meetings. Similar to any organization, there is a need for anticipations, vivid missions, team building, setting goals, and planning, which ensures a smooth running.Advertising We will write a custom essay sample on Organizational Behavior: the Family, College Class, and Organization specifically for you for only $16.05 $11/page Learn More Hence, every family member should possess a particular role. In a class college, organization, and family, the job description is imperative in defining the members’ obligations and roles. Moreover, a clear job description promotes more input from individuals, which gives the members a sense of ownership. The family, college class, and organization are characterized by universality. The three are present in all human society levels, everywhere, and always. In the three, the me mbers are united by a common goal. Hence, there is some form of emotional basis. In the family, people are united by affection and mutual love, which enhances sympathy and empathy towards each other. It is evident that in the class and organization, members have to collaborate to fulfill the set goals, which unites them. Another similarity between the three is the limited size. Management Roles The family council comprises of the family members. In a college class, the council constitutes of the entire class and class teacher. Finally, the employees and management comprise the organization council. In a family, the male parent has the responsibility of governing the family. The female parent assists the male parent in running the family. In a college, the class teacher oversees the overall running of the class. The class prefect, who has a closer relationship with the students, ensures maintenance of order. In an organization, the manager is the overall overseer. The success of an o rganization, class, and family depends on regular meetings. In a meeting, members get the opportunity to be heard, distribute responsibilities, receive encouragement, congratulate exemplary roles, set goals, share, plan for events, solve conflicts and recurring issues, set objectives, and express complaints and concerns.Advertising Looking for essay on business economics? Let's see if we can help you! Get your first paper with 15% OFF Learn More Leaders in the three organizations have to ensure that the appropriate leadership style is used. Depending on different circumstances, it might be necessary to change the leadership style. Moreover, leaders have to engage in critical controlling, organizing, and planning. The available resources should be dedicated towards goal achievement. How Diversity Contributes to Efficiency and Effectiveness Diversity in the family, organization, and college class ensures that effectiveness and efficiency are achieved. To ensur e that diversity is achieved, there is a need for constant role rotations. For instance, the secretary and manager roles should be rotated after a certain period. It is worth noting that every member in an organization is gifted differently. Therefore, there is a need to give everyone the opportunity to contribute towards diversity. Furthermore, every member should be given an opportunity to voice their ideas. Scheduling weekly meetings ensures every member presents updates from their departments, and that all pressing issues are discussed. The meetings should be evaluated regularly, and openness and mutual respect should be upheld. When families visit their family friends, they get an opportunity to learn new things and skills. Sometimes class competitions assist classes to learn new ways of doing things. It is worth emphasizing that diversity comprises of one’s background, cognitive style, gender, and race. The way members in an organization perceive others is extremely imp ortant. Therefore, the human resource management should deal with transformations, adaptability, and communication.

Ionization Energy Definition and Trend

Ionization Energy Definition and Trend Ionization energy is the energy required to remove an electron from a gaseous atom or ion. The first or initial ionization energy or Ei of an atom or molecule is the energy required to remove one mole of electrons from one mole of isolated gaseous atoms or ions. You may think of ionization energy as a measure of the difficulty of removing electron or the strength by which an electron is bound. The higher the ionization energy, the more difficult it is to remove an electron. Therefore, ionization energy is in indicator of reactivity. Ionization energy is important because it can be used to help predict the strength of chemical bonds. Also Known As: ionization potential, IE, IP, ΔH ° Units: Ionization energy is reported in units of kilojoule per mole (kJ/mol) or electron volts (eV). Ionization Energy Trend in the Periodic Table Ionization, together with atomic and ionic radius, electronegativity, electron affinity, and metallicity, follows a trend on the periodic table of elements. Ionization energy generally increases moving from left to right across an element period (row). This is because the atomic radius generally decreases moving across a period, so there is a greater effective attraction between the negatively charged electrons and positively-charged nucleus. Ionization is at its minimum value for the alkali metal on the left side of the table and a maximum for the noble gas on the far right side of a period. The noble gas has a filled valence shell, so it resists electron removal.Ionization decreases moving top to bottom down an element group (column). This is because the principal quantum number of the outermost electron increases moving down a group. There are more protons in atoms moving down a group (greater positive charge), yet the effect is to pull in the electron shells, making them smaller and screening outer electrons from the attractive force of the nucleus. More electron shells are added moving down a group, so the outermost electron becomes increasingly distance from the nucleus. First, Second, and Subsequent Ionization Energies The energy required to remove the outermost valence electron from a neutral atom is the first ionization energy. The second ionization energy is that required to remove the next electron, and so on. The second ionization energy is always higher than the first ionization energy. Take, for example, an alkali metal atom. Removing the first electron is relatively easy because its loss gives the atom a stable electron shell. Removing the second electron involves a new electron shell that is closer and more tightly bound to the atomic nucleus. The first ionization energy of hydrogen may be represented by the following equation: H(g) → H(g) e- ΔH °Ã‚   -1312.0 kJ/mol Exceptions to the Ionization Energy Trend If you look at a chart of first ionization energies, two exceptions to the trend are readily apparent. The first ionization energy of boron is less than that of beryllium and the first ionization energy of oxygen is less than that of nitrogen. The reason for the discrepancy is due to the electron configuration of these elements and Hunds rule. For beryllium, the first ionization potential electron comes from the 2s orbital, although ionization of boron involves a 2p electron. For both nitrogen and oxygen, the electron comes from the 2p orbital, but the spin is the same for all 2p nitrogen electrons, while there is a set of paired electrons in one of the 2p oxygen orbitals. Key Points Ionization energy is the minimum energy required to remove an electron from an atom or ion in the gas phase.The most common units of ionization energy are kilojoules per mole (kJ/M) or electron volts (eV).Ionization energy exhibits periodicity on the periodic table.The general trend is for ionization energy to increase moving from left to right across an element period. Moving left to right across a period, atomic radius decreases, so electrons are more attracted to the (closer) nucleus.The general trend is for ionization energy to decrease moving from top to bottom down a periodic table group. Moving down a group, a valence shell is added. The outermost electrons are further from the positive-charged nucleus, so they are easier to remove. References F. Albert Cotton and Geoffrey Wilkinson, Advanced Inorganic Chemistry (5th ed., John Wiley 1988) p.1381.Lang, Peter F.; Smith, Barry C. Ionization Energies of Atoms and Atomic Ions. Journal of Chemical Education. 80 (8).