Question

1. What is the total number of electrons that occupy a shell, n?

2. List the relative energies for the different subshells.

3. What are the relative energies of orbitals within a shell?

4. How many electrons can be accommodated in each orbital orientation?

5. How many s-orbitals are there in a shell?

6. How many p-, d- and f- orbitals are there in a given shell?

7. What is an abbreviated or condensed electron configuration?

8. Why is it important to identify valence electrons?

9. Define:

-Transition metals

-Main group elements

10. How do metallic behavior and electron configuration relate?

11. How does one specifically determine the anomalous configurations of transition

and inner transition elements?

12. How does electron configuration relate to atomic properties?

13. What is the atomic radius (bonding atomic radius or covalent radius)?

14. What must you consider when comparing atoms for size (radius)?

15. What is ionic radius?

16. What must you consider when comparing ions for size?

17. How do you determine the magnetic properties of an atom?

18. What are successive ionization energies?

19. What are the trends in the second ionization energy?

20. What is oxidation? Reduction?

21. What is the trend for metallic reactivity? What is its trend on the periodic table?

22. What is the trend for the nonmetallic character? What is its trend on the periodic

table?

23. What is electronegativity? What is its trend on the periodic table?

Answer 1

1. Shell N can have 4s 2 electron 4p 6electron 4d 10 Electron and 4f 14 electron which sums upto 32 electrons. The general formula is that the nth shell can in principle hold up to 2(n2) electrons.

2. In a shell, the order of energy is s<p<d<f.

3. The 1s subshell has the lowest relative energy

The 2s subshell has the second lowest relative energy, followed by the 2p subshell.

In the 3rd shell, the 3s subshell has the lowest relative energy, followed by the 3p subshell. After this, the 4s subshell as it has a lower relative energy than the 3d subshell. The 3d subshell is afterwards, followed by the 4p, then 4d, then 4f. The filling of electron depend upon the energy levels of diffrent subshells therefore the relative energy of a subshell can also be estimated.

4.1s can hold 2 electron. 2p hold 6 electron. 3d can hold 10 electron and 4f can hold 14 electron.

5. Each shell has one s- orbital

6. There are only one p, d and f orbital in a given shell. (azimuthal quantum number ℓ describes the orbital angular momentum of each electron doesn't repeats in a shell)

7. The abbreviated electron configurations uses Noble gas configurations, which have full electron shells, to describe the electronic structure of later elements.

8. Valence electrons are the electrons that reside in the outermost electron shell of an atom in the highest energy level. They are important because the number of valence electrons the atom holds the more stable it is. In addition to that, the amount of valence electrons in the outer shell determines how atoms interact with one another.

9. The transition metals are a group of metals that are found in the middle of the periodic table. They all have similar properties. The alkaline earth metals, beginning with beryllium are to the left and the boron group elements are to the right. They are harder and less reactive than the alkaline earth metals. They are also harder than the post transition metals. They make colorful chemical compounds with other elements. Most of them have more than one oxidation state. Like other metals, they are electrical conductors.

The main group is the group of elements (sometimes called the representative elements) which includes the elements (except hydrogen, which is sometimes not included) in groups 1 and 2 (s-block), and groups 13 to 18 (p-block). The s-block elements are primarily characterised by one main oxidation state, and the p-block elements, when they have multiple oxidation states, often have common oxidation states separated by two units.

13. The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding shells of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius. Three widely used definitions of atomic radius are: Van der Waals radius, ionic radius, and covalent radius.

14. We must always be comparing the radius under same category like covalent to covalent not ionic to covalent.

15. The ionic radius is the measure of an atom's ion in a crystal lattice. It is half the distance between two ions that are barely touching each other

16 Anions are generally bigger than cations so one should always consider it.

17. The magnetic property of a substance can be determined by examining its electron configuration: if it shows unpaired electrons, then the substance is paramagnetic; if all electrons are paired, the substance is diamagnetic.

18. Ionisation energy is the energy required to remove an electron from the outermost shell of an isolated gaseous atom. When the first electron or the most loosely bound electron is removed, the amount of energy required is less than the energy required to remove the electron in the next successive shell. This ionisation energy goes on increasing with the number of electrons removed. So the number of electrons removed from the successive no of shells and the energy involved is called successive ionization energy.

19. 2nd ionization energy - The energy required to remove a second electron from a singly charged gaseous cation.

20. Oxidation is the loss of electrons during a reaction by a molecule, atom or ion. Oxidation occurs when the oxidation state of a molecule, atom or ion is increased. The opposite process is called reduction, which occurs when there is a gain of electrons or the oxidation state of an atom, molecule, or ion decreases.

21.

22.

24. Electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons (or electron density) towards itself.