Chemistry
Use the letters only written in the Periodic Table given below to answer the questions :
| I | II | III | IV | V | VI | VII | O | |
|---|---|---|---|---|---|---|---|---|
| 1 | L | |||||||
| 2 | Q | E | G | J | Z | M | ||
| 3 | R | |||||||
| 4 | T |
(i) State the number of valence electrons in atom J.
(ii) Which element shown forms ions with a single negative charge?
(iii) Which metallic element is more reactive than R?
(iv) Which element has it's electrons arranged in four shells?
Answer
(i) Atom J has 5 valence electrons as it belongs to the fifth group in the periodic table.
(ii) M forms ions with a single negative charge as it has 7 electrons in the valence shell and obtaining one more electron completes it's octet.
(iii) Metal T is more reactive than R because elements at the bottom of the group are more reactive.
(iv) T has it's electrons arranged in 4 shells as it belongs to 4th period.
Related Questions
Identify the term in each of the following :
(i) The tendency of an atom to attract electrons to itself when combined in a compound.
(ii) The electrons present in the outermost shell of an atom.
Write the correct symbol > (greater than) or < (less than) in the statements :
(i) The ionization potential of potassium is ………. that of sodium.
(ii) The electronegativity of iodine is ………. that of chlorine.
Fill in the blanks by selecting the correct word :
(i) If an element has a low ionization energy then it is likely to be ………. (metallic/non metallic).
(ii) If an element has seven electrons in it's outermost shell then it is likely to have the ………. (largest/smallest) atomic size among all the elements in the same period.
Select the correct answer — The energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion is called ………. (electron affinity, ionization potential, electronegativity)