Explain how elements are arranged in the periodic table, in relation to atomic number and groups and periods.
Answers
Answer:
The chemical elements are arranged in order of increasing atomic number. The horizontal rows are called periods and the vertical columns are called groups. Elements in the same group have similar chemical properties. This is because they have the same number of outer electrons and the same valency.
numbered 1–18 from left to right); the seven horizontal rows are called periods.
The number of valence electrons in the atom determines the group number of that atom i.e. if an element has 4 valence electrons then it must belong to group IV A. Since sodium has 3 shells, it belongs to period 3.
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1.In the modern periodic table, the elements are listed in order of increasing atomic number.
2.The elements having similar chemical properties naturally line up in the same column (group).
3.For instance, all of the elements in Group 1A are relatively soft metals, react violently with water, and form 1+ charges; all of the elements in Group 8A are unreactive, monatomic gases at room temperature, etc.
4.In other words, there is a periodic repetition of the properties of the chemical elements with increasing mass.
5.numbered 1–18 from left to right); the seven horizontal rows are called periods
Explanation:
1.The atomic number is the number of protons in the nucleus of an atom. The number of protons define the identity of an element (i.e., an element with 6 protons is a carbon atom, no matter how many neutrons may be present).
2.The number of protons determines how many electrons surround the nucleus, and it is the arrangement of these electrons that determines most of the chemical behavior of an element.
3.The modern periodic table is arranged in groups and periods based on the electronic configuration of the atoms of elements.
4.Physical and chemical properties of elements are related to their electronic configurations particularly the outershell configurations.