periodicity Flashcards
what happens to metal reactivity as you move across a period
decreases because has a higher electronegativity meaning that it wants to be more stable
what happens to metal reactivity as you move down a group
increases because of electron shielding allowing for a lower first ionisation energy
what happens to metal reactivity as you move up and across the periodic table
decreases across because less electron shielding and higher electronegativity = lower first ionisation energy and higher tendency to be stable
increases down as lower ionisation energy
what happens to core charge as you move across a period
increases as there are more valence electrons, therefore a higher core charge
what happens to electronegativity as you move across the periodic table
electronegativity increases as you move across the periodic table because there are more valence electrons
what is the first ionisation energy
First ionization energy is the amt of energy required to remove the first valence electron from the gaseous state.
specify gaseous state
define melting point
the temperature of which it takes a substance to go from solid to liquid
what is electronegativity
an elements tendency to attract electrons
in what direction of the periodic table does atomic radius increase
bottom left
what are characteristics of the s block
alkali metals, soft, low melting points, electropositive
what are characteristics of the p block
forms covalent compounds, losing and gaining electrons
what are characteristics of the d block
transition metals, different charges for the same elements, behave either like highly reactive electropositive alkali metals
or covalent compound forming elements
what are characteristics of the f block
high melting points
define core charge
Core charge of an atom is a measure of the attractive force experienced by the valence electrons towards the nucleus.
