gcse chemistry C1

• The reactivity series is used to predict which metal will displace another from its compound.
• Metals are arranged on the periodic table by their atomic number, with metals having low electronegativity values (less than 2) being more reactive.
• Reactivity increases down groups due to an increase in metallic character and decrease in ionization energy.
• A more reactive metal displaces a less reactive one, as it has a higher reduction potential (more positive).
• Metals are arranged in the periodic table by their atomic number, with metals on the left being more reactive than those on the right.
• Group 0 elements have low melting points due to weak intermolecular forces between molecules.
• Reactivity decreases across periods as there is less space between atoms, making it harder for them to lose electrons.
• Alkali metals have one electron in their outer shell and readily form +1 ions when they gain an electron.
• Alkaline earth metals have two electrons in their outer shell and readily form +2 ions when they gain two electrons.
• In the reaction between copper sulfate solution and zinc granules, copper(II) ions are reduced to copper metal while zinc atoms are oxidized to Zn2+ ions.
• Increasing size within a group leads to decreased melting point and increased boiling point due to weaker intermolecular forces between larger atoms.
• Group 7 elements have similar properties because they all contain seven valence electrons.
• Copper metal is produced at the cathode during electrolysis of molten copper(Ii) chloride using carbon rods as electrodes.
• Increasing size within a group leads to weaker intermolecular forces, resulting in lower boiling points.
• Electron configuration determines whether an element can form ions or not.
• Electroplating involves passing an electric current through a solution containing dissolved metal ions to deposit them onto a solid object.
• The reactivity series can be used to predict which element will displace another from its compound when heated together.
• The reactivity series shows how easily a metal can be oxidized or reduced under standard conditions.
• Elements in Group 7 have high melting and boiling points because they form strong covalent bonds.
• Alkali metals are very reactive because they easily lose electrons to form positively charged ions.
• As the size of atoms decreases across a period, there is a greater attraction between nuclei and valence electrons, leading to stronger bonding and higher melting/boiling points.
• The reactivity series can be used to predict which metal will displace another from its compound.
• Increasing atomic radius leads to weaker metallic bonds and lower melting/boiling points.