Atomic Radius and Atomic Structure

1-Describe the periodic trend in atomic radius and relate it to atomic structure 2- Describe the periodic trend in electronegativity and relate it to atomic structure Did you know?
There are atoms with no electronegativity because electro negativity refers to the attraction of atoms of electrons in a compound; elements that do not form are assigned no electronegativity values. Atomic Radius ≠ Ionization Energy

As you move from left to right on the periodic table, the number of valance electron increase. As the number of E increases P increases. As positive force increases, the electron get tighter and the radius gets smaller. Ionization energy is the energy required to remove an electron. As you move up and down the periodic table, the number of electron shells changes. As the number of shells increases, there is more shielding between the nucleuses the outermost electron increases. Atomic Radius: is half the distances between 2 identical atoms that are bonded. It is the distance between the nucleus and the outer shell.

Electro negativity:
When atoms are bonded together, unless they are 2 identical atoms, one of those atoms is always going to be better at attracting electrons to it. Electronegativity: is the ability of an atom to attract electrons to itself. Electronegativity: will increase when it goes from left to right and down to up and will decrease when decreases goes from right to left electronegativity and up to down. Atomic radius: decreases from left to right and down to up, and increases from right to left and up to down. Ionization Energy: will increase when it goes from left to right and down to up and will decrease when decreases goes from right to left electronegativity and up to down. As we move fro, left to right on the periodic table the atomic radius decreases, and as it decreases, the nucleus is better able to attract electrons to it. So, electronegativity increases going from left to right. As you move from top to bottom, the atomic radius increases. As it increases, the number of inner shells increases. As it increases the nucleus is less able to attract electrons to it. Chapter4 section 3

Melting point: is the temperature at which a substance turns to a liquid from a solid. Boiling point: is the temperature at which a substance turns to gas from a liquid. The metals have high melting and boiling point because they are solids at room temperature Gases and liquids have low melting points and boiling points because they are liquids and gases at room temperature.

Chapter 5 section 1

Objectives:
1) Determine an atoms number and valance electrons, and use the octet rule to predict what stable ions the atom is likely to form.

The ions on the periodic table have the same electron configuration as the noble gases. This happens because elements form ions in such a way that they will achieve a noble gas electron configuration.

The transition metals can have multiple charges when they form positive ions each metal can have more than one possible charge. The charge that it will carry depends on the conditions. The transition metals do not form ions in a way that will achieve a noble gas electron configuration.