The trends from left to right in a period increase (nuclear charge), and moving down a group decreases (shielding).
Electronegraitive Periods and groups are atomic radius decreases as you go from left to right across a period.
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.
carbon (group 14, period 2) hydrogen (group 1, period 1) nitrogen (group 15, period 2) oxygen (group 16, period 2) sulphur (group 16, period 3) halogens (group 17, period 2-5)
um not really sure but like lithium or something
Group number 12, period number 4 Transition metal
The group that is usually ignored because it does not follow trends is often referred to as the "nonconformists" or the "individualists." These individuals choose to go against popular trends and are often overlooked or dismissed because of their uniqueness and refusal to conform. However, their perspectives and ideas can bring fresh and innovative insights that should not be ignored.
Electron Configuration
The atomic radius decreases along the elements across a period. Along a group, there is an increment in the atomic radius of corresponding elements.
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.
Increase
Down the group electron affinity decreases Across a period electron affinity increases. However, it should be noted that chlorine is having higher electron affinity than flourine due to the small size of fluorine atom)
In general, they are opposing. Electronegativity increases going left to right in a period and up in a group. Atomic radius decreases going left to right in a period and up in a group.
From left to right on the periodic table, ionization energy increases. From top to bottom in a column (group) the ionization energy decreases.
The periodic trends that arise from the arrangement of the periodic table provide chemists with an invaluable tool to quickly predict an element's properties. These trends exist because of the similar atomic structure of the elements within their respective group families or period and the periodic nature of the elements.
Carbon is in group 14, period 2
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.
The Noble Gases