Advertisements
Advertisements
Question
The number of electrons in the outermost shell of alkali metals is ______.
Options
1
2
3
7
Advertisements
Solution
The number of electrons in the outermost shell of alkali metals is 1.
Explanation:
Alkali metals belong to Group 1 of the periodic table, which includes elements like lithium, sodium, and potassium. They all have a valence electronic configuration of (ns1). Because they possess exactly one electron in their outermost shell, they easily lose it to form univalent positive ions (M+) and achieve a stable noble gas configuration.
APPEARS IN
RELATED QUESTIONS
Why do we classify elements?
An element Y is in second period and group 16 of the periodic table:
(i) Is it a metal or non-metal?
(ii) What is the number of valence electrons in its atom?
(iii) What is its valency?
(iv) What is the name of the element?
(v) What will be the formula of the compound formed by Y with sodium?
As element X has mass number 40 and contains 21 neutrons in its atom. To which group of the periodic table does it belong?
The element X forms a compound X2Y. Suggest an element that Y might be and give reasons for your choice.
What is the need for classification of elements?
State whether true or false. If false, correct the statement.
Metals can gain electrons.
Match the following
| 1. | Galvanisation | Noble gas elements |
| 2. | Calcination | Coating with Zn |
| 3. | Redox reaction | Silver-tin amalgam |
| 4. | Dental filling | Alumino thermic process |
| 5. | Group 18 elements | Heating in the absence of air |
Identify the bond between H and F in the HF molecules.
An element X from group 2 of the Periodic Table reacts with Y from group 17 to form a compound. Give the formula of the compound.
Which one of the following does not increase while moving down the group of the periodic table?
In which group are inert elements placed?
Which of the following property will be common in group 1 elements?
The element with atomic number 26 will be found in group ______
Arrange the following elements in the order of their decreasing metallic character
Na, Si, Cl, Mg, Al
An element is placed in 2nd Group and 3rd Period of the Periodic Table, burns in presence of oxygen to form a basic oxide.
- Identify the element
- Write the electronic configuration
- Write the balanced equation when it burns in the presence of air
- Write a balanced equation when this oxide is dissolved in water
- Draw the electron dot structure for the formation of this oxide
Complete the following triads by inserting the missing elements.
Cl, ______, I
Identify the following:
An element in Period 1 which can be placed in both Group 1 and Group 17 of the Periodic Table.
Element 'X' forms an oxide with the formula X2O3 which is a solid with high melting point. ‘X’ would most likely be placed in the group of the Periodic Table as:
Justify. Element 'X' forms an oxide with the formula X2O3 which is a solid with a high melting point. ‘X’ would most likely be placed in the group of the Periodic Table as Al.
