Chemistry - Periodic Table Flashcards
what are the key properties of the periodic table?
electronegativity
atomic radius
ionisation energy
electron affinity
describe electrogativity
see lesson 7
the measure of the attraction of an atom for the electrons in a chemical bond. the higher the electronegativity, the greater its attraction for bonding electrons
describe atomic radius
see lesson 7
the measure of attraction of an atom for the electrons chemical bond. the higher the electronegativity the greater its attraction for bonding electrons
what are the classifications of different metals
alkali
alkali earth
metalloids
non metals
transition metals
halogens
noble gases
what are alkali metals, give examples
soft shiny metals that are extremely reactive, only have one valence electron
what are alkali earth metals, give examples
slightly harder and less reactive, only have two valence electrons
what are non metals, give examples
gaseous and tend to gain electrons and fill their valence shells
what are metaloids, give examples
have some metallic properties
what are transition metals, give examples
solid at room temp, except mercury, and have their metallic colour and malleability expected of metals
what are halogens , give examples
have the ability to produce salts
what are noble gases, give examples
far right on the periodic table and have full valence shell and tend to neither loose or gain electrons
how do we read elements on the periodic table?
using the atomic no., element name, atomic mass and symbol
how do elements combine?
see lesson 7
through ionic and covalent bonds
ionic -
attractive force that forms when one or more electrons is transferred from one atom to another
covalent -
a force holding to atoms together by sharing electrons
how do we balance equations?
practice, see lesson 7
