Trends in the Periodic Table: ionisation energy, electronegativity, atomic radius, melting and boling poins

Ionisation energy is the energy to remove the first negatron from an fragment in the gaseous state. - Increases crossways a pointedness as electron shells go from near empty to overflowing. - Decreases down(p) a group as the outer electrons become further hostile from the unconditional nucleus. - The second ionisation energy is always big than the first since the electron is now being removed from a positive ion. Electronegativity is the relative power to attract electrons. - Increases across a period as the lean of protons increases so does the positive indicate of the nucleus, thus a stronger attraction and electrons are being held much tightly. - Decrease down a group as the invalidatingly charged electrons repel each other and the invaders. The more than protons, the great the number of occupied electron shells that shield the nucleus. - degree Fahrenheit is the well-nigh electronegative element and when combined with caesium, will move violently. Atomic R adius - Decreases across a period because the number of positively charged protons in the nucleus increases, pulling the negative electrons in more tightly. - Increases down a group as the number of electron shells increase.

Melting and turn Points - Increases to root word IV, consequently rapidly decreases. - Groups I and II (Metallic bond). chasten to high - Group IV (Covalent network solids). Very high - Group seven (Diatomic covalent). Forces between molecules are weak so its low. - Group eight (Monatomic gases). Only forces between atoms are weak dispersion forces so its very low If you want to get a full es! say, bon ton it on our website: OrderCustomPaper.com

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