Electronegativity, electron affinity, nonmetalic nature, acidic nature of oxides, valency with respect to oxygen ( from 1 to 7), number of electrons in the outer most shell ( 1 to 8) increases across a period from left to right
Atomic radius decreases across a period. This is due to increase in nuclear charge.
Metallic properties decreases across a period. Non-metallic character increases.
- the atomic weight
- the number of protons
atomic radius and ionization energy
metal and non-metal and nobel gasses
Several exceptions exist for this rule.
atomic mass, triads, and octaves
The atomic radius of Na is greater than that of Si because as you move to the right across the periodic table there are more electrons which cause more attraction between the protons and electrons which cause them to pull closer together.
Atomic size generally increases as you go down a group
The size of an atom refers to its atomic radius. Atomic radius generally increases down a group. This is because the number of energy levels increase down a group with each additional period. Each of the subsequent energy levels are larger than the last, increasing the distance of the electrons from the nucleus, which increases the atomic radius.Atomic radius generally decreases across a period. This is because electrons are being added to the same energy level at the same time that protons are being added to the nucleus. This creates a stronger force of attraction by the nucleus for the electrons, which pulls the electrons closer to the nucleus, decreasing the atomic radius.It is important to note that the periodic trends are not laws. There are exceptions to the general trends in both the representative elements and the transitional elements.
Overall as atomic number increases covalent radius increases.
The atomic number increases from left to right. The atomic number also increases.However, there are few exceptions for atomic mass.
Atomic radius increases down the group. It decreases along a period.
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.
Atomic Mass increases in size as the atomic number increases. For example, hydrogen weighs about 1.01 grams per mole and it has periodic #1. Helium is atomic #2 and it has an atomic mass of 4.00 g/mol. This trend continues all the way to the last known pure element.
For periodic trends we will examine1- Electronic configuration 2- Ionization energy 3- Atomic radius
well, the periodic table is very useful because you have the atomic number, atomic mass, and even the trends across a period or down a group.
Atomic Mass Octaves and Triads
atomic mass, triads, and octaves
The atomic radius of Na is greater than that of Si because as you move to the right across the periodic table there are more electrons which cause more attraction between the protons and electrons which cause them to pull closer together.
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Atomic size decreases from left to right in a period hence ioniztion energy increases from left to right.But atomic size increases from top to bottom in a group hence ionization energy decreases from top to bottom.
Atomic size generally increases as you go down a group