periodic trends The periodic table is often considered to be the \"best friend\"
ID: 712042 • Letter: P
Question
periodic trends The periodic table is often considered to be the "best friend" of chemists and chemistry It ineludes information about atomic masses and element symbols, but it can also be used to Workshop 4: Periodic Trends make predictions about atomic sizes, electronegativity, lonization energies, bonding, solubility or reactivity. Today's workshop is all about understanding ionization energy (lE) energy required to remove the outermost electron from an atom to create a m an atom/ion one at a time and so most atoms to remove IE is the amount of tion energy. Each successive ionization energy the IE ion. E ectrons are always removed fro all except hydrogen) will have more than 1 ioniza for a given element represents the removal of a subsequent electron The table below contains the first 4 ionization energies of magnesium. Our goal is to write equations for all four lE values, but before we do that, let's make sense of the values in the table. 696 1752 kl/mol 14,807 kl/mol 17,948 k/mol 1. it is often said that all of chemistry is governed by electrostatic interactions. What do you think holds the electrons of Mg to its nucleus? 2 Why do you think the ionization energy for Mg increases as you go from li to 142 3. Why do you think there is such a large difference between the 2al and 3d ionization energies of Mg? Now certify: Can all members answer these questions independently: all members sign below and then nove on to solving the problem. names hereExplanation / Answer
Part 1
1. The nucleus of a neutral Mg atom contains protons and neutrons. The protons are positively charged while the neutrons are negatively charged. Hence, the nucleus is a small region of the atom (central part) having high positive charge density. The electrons are negatively charged and revolve around the nucleus in orbits. The electrons are attracted to or bound to the nucleus by the electrostatic force of interaction between opposite charges. Basically, the positively charged nucleus and the negatively charged electrons are held together by an electric force that operates between opposite charges.
2. The electronic configuration of Mg is given as
Mg (12): 1s22s22p63s2
The valence electrons of Mg are in the 3s orbital. Removal of these two electrons is easy as Mg has an inherent tendency to lose these two electrons to attain the stable inert gas configuration of Ne (atomic number 10, electronic configuration 1s22s22p6). Formation of Mg2+ is rather easy and hence, IE1 and IE2 are low. However, IE3 and IE4 involve breaking up of the stable inert gas configuration and hence, are highly energy-demanding processes and hence, the 3rd and 4th ionization energies of Mg are extremely high.
3. It has already been noted above that IE3 and IE4 of Mg are high since these involve breaking the inert gas shell configuration. Moreover, the 2p orbitals in Mg2+ are full-filled and full-filled (also half-filled) orbitals are unusually stable; hence, there is a large difference between IE2 and IE3.
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