Admin Table of Contents
- 1 Why the position of hydrogen can be placed either in Group 1 or Group 17 in the first period?
- 2 Why has hydrogen been placed in the first group of the periodic table although it is a non metal?
- 3 Why is it difficult to place hydrogen in the modern periodic table?
- 4 Why are members of Group 1 called alkali metals?
- 5 Which element of Group 1a is not an alkali metal and why?
- 6 What is the electron configuration for Group 1a?
- 7 What is the electronic configuration of Group 1 elements?
- 8 How do you find similar electron configurations in a group?
Why the position of hydrogen can be placed either in Group 1 or Group 17 in the first period?
Hydrogen can be placed in both group 1 and group 17 because its electronic configuration is similar to both the groups. However, like group 17 elements, it requires only electron to complete its valence shell, thus it can also gain an electron to achieve a noble gas configuration.
Why has hydrogen been placed in the first group of the periodic table although it is a non metal?
Hydrogen is a non metal but as per the electronic configuration there is the arrangement of the electrons and the elements with one electron in the outer most shell is placed in the 1st group. so hydrogen is also placed for the same.
Is H part of group 1A?
Group 1A — The Alkali Metals. Group 1A (or IA) of the periodic table are the alkali metals: hydrogen (H), lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). These are (except for hydrogen) soft, shiny, low-melting, highly reactive metals, which tarnish when exposed to air.
Why does hydrogen not fit into this group?
Hydrogen is therefore arguably the most important element for life, but can we fit it into a group in the periodic table? It does not readily form H+ cations and forms covalent bonds in most compounds, whereas group 1 metals readily form cations and form only ionic bonds.
Why is it difficult to place hydrogen in the modern periodic table?
It is difficult to decide where hydrogen belongs in the periodic table because of the physical properties of the element. Hydrogen also has an electronegativity (EN = 2.20) halfway between the extremes of the most electronegative (EN = 3.98) and least electronegative (EN = 0.7) elements.
Why are members of Group 1 called alkali metals?
The Group 1 elements are called the alkali metals. All the Group 1 elements are very reactive . They must be stored under oil to keep air and water away from them. Group 1 elements form alkaline solutions when they react with water, which is why they are called alkali metals.
Why hydrogen could be placed in either Group 1 or group 7?
Hydrogen has been placed in Group 7A (IUPAC Group 17), because — just like elements in that group — it is monovalent in common compounds and requires just one electron to fill its outer shell.
Why is hydrogen on the periodic table with the metals in Group 1?
Why is hydrogen, a nonmetal, placed in the same group as the alkali metals? Because it has eight valence electrons like all the other elements in group 1. Because it has just one valence electron like all the other elements in group 1. Because it has two valence electrons like all the other elements in group 1.
Which element of Group 1a is not an alkali metal and why?
hydrogen
(Like the other elements in Group 1, hydrogen (H) has one electron in its outermost shell, but it is not classed as an alkali metal since it is not a metal but a gas at room temperature.) Brush up on the periodic table of elements.
What is the electron configuration for Group 1a?
18.2: Group 1A Metals
| Element | Symbol | Electron Configuration |
|---|---|---|
| Lithium | Li | [He]2s1 |
| Sodium | Na | [Ne]3s1 |
| Potassium | K | [Ar]4s1 |
| Rubidium | Rb | [Kr]5s1 |
Why is hydrogen not placed in Group 1 even though it has 1 valence electron?
Hydrogen is a nonmetal and is placed above group in the periodic table because it has ns1 electron configuration like the alkali metals. However, it varies greatly from the alkali metals as it forms cations (H+) more reluctantly than the other alkali metals.
Why hydrogen could be placed in either Group 1 or Group 7?
What is the electronic configuration of Group 1 elements?
Electronic Configuration of Group I Elements. Electronic configuration represents that the ultimate shells of the alkali metals do have one s electron (S 1 electron) while in the penultimate shells there are eight electrons S 2 P 6 except for the Lithium.
How do you find similar electron configurations in a group?
It is easy to see how similar electron configurations are in a group when written out. (Allow “n” to be the principal quantum number.) Lets first take a look at group 1 atoms. Group 1 atoms are the alkali metals. Let n=1. Notice the similar configuration within all the group 1 elements. Now consider group 16 elements.
What is the electronic configuration of an atom?
Electronic Configuration of Group 1 and Group 2 Elements The electronic configuration of an atom is the represents the arrangement of the electrons distributed among the shells and subshells. In other words, electronic configuration describes how the electrons are assembled in the shells and subshells of the atoms.
What is the outermost electronic configuration of the s block elements?
Hence, the outermost electronic configuration of the s block elements is ns 1 or ns 2 as all the inner orbitals are completely filled. In the modern periodic the s block elements have been placed in the first two groups that are the group I (alkali metals) and group II (alkaline earth metals).