M1 Topic 3 part 2: Periodicity (ionisation energy, electronegativity, reactivity with water) Flashcards
What is electronegativity
The measure of the ability of an atom to attract electrons while it is part of a compound
What is the trend of electronegativity across the periodic table
Electronegativity generally increases , as shells are drawn closer to the nucleus as they become more even
Why do the shells in group 18 get bigger instead of smaller
This is because due to the outer shell being fully valent with these element, it allows the outer shell to propel away from the nucleus
What is the trend in electronegativity down the periodic table
Electronegativity becomes lower and elements become more reactive
Why does electronegativity get lower down the periodic table
It’s because the outer shell gets further away every time you go down making it less affected by the nucleus
what is ionisation energy
energy required to remove an electron from an atom
what is 1st energy
energy needed to remove the first electron
what happens when you do successive ionisation
energy increases as the remaining electrons feel stronger attraction to the resulting cation produced
what is the general trend of ionisation
generally decreases down a group and increases left to right across a period
which elements react with cold water (3)
K: potassium
Na: sodium
Ca: calcium
which elements react with hot water(1)
mg: magnesium
which elements react with steam(3)
Al: aluminium
Fe: iron
Zn: zinc
what is the equation for an elements that reacts with cold water
(metal) + H2 0(aq) –> H2 + metal OH-
what is the equation for magnesium reacting with hot water
Mg + 2H2 0 (aq), (hot) –>h2 + Mg(OH)2
what is the equation for elements reacting with steam
(metal)+ H2 O(g) –> H2 + (metal)O
