Chemistry Paper 1 🧪

• properties of metals?

  -strong

  -malleable

  -conductors of heat and electricity -high boiling and melting point

  -metallic bonding
• properties of non-metals?

  -dull

  -brittle

  -lower density

  -don’t conduct electricity
• properties of transition metals?

  -dense

  -strong

  -shiny

  -conductor of heat and electricity
• properties of group 1 elements?

  -soft

  -low density

  -very reactive

  -1 electron in outer shell
• trends going down group 1?

  -lower melting and boiling point

  -reactivity increases
• why does reactivity increase down group 1?

  -outer electron is lost more easily

  -as attraction between nucleus and electron decreases as you go down
• what compounds and ions do group 1 form?

  -ionic compounds

  -1 + ions
• what happens when group 1 react with water?

  -react vigorously

  -produce metal hydroxide and hydrogen gas
• what happens when group 1 react with chlorine?

  -vigorous reaction

  -form white metal chloride salts
• what happens when group 1 react with oxygen?


  -form metal oxides
• differences between group 1 and transition metals?

  -group 1 are more reactive, less dense, and have lower melting points
• trends going down group 7?

  -higher melting and boiling points

  -less relative atomic mass

  -less reactive
• why are elements in group 7 less reactive as you go down?

  -it’s harder to gain an extra electron because outer shell is further from nucleus

  -so there’s less attraction
• what compounds do group 7 form?


  -molecular compounds that have simple molecular structures
• what is a simple molecular structur?

  -molecules containing a few atoms joined together by covalent bonds
• what bonds and ions do group 7 form with metals?

  -ionic bonds

  -1 negative ions
• what can a more reactive halogen displace?

  -a less reactive halogen from an aqueous solution of its salt
• what are group 0 elements?

  -inert

  -non flammable

  -monatomic
• trends going down group 0?

  -boiling point increases
• why does the boiling point increase down group 0?

  -the number of electrons in each atom increases so there are greater intermolecular forces that need to be overcome
• why are group 0 unreactive?

  -8 electrons in outer shell so they’re stable

  -this means they don’t have to lose or gain any electrons to have a full outer shell
• metals to the left of the periodic table…?

  -don’t have many electrons to remove
• metals towards the bottom of the periodic table…?

  -have outer electrons far from nucleus so weaker attraction
• non-metals to the right of the periodic table…?

  -have lots of electrons to remove
• metals towards the top of the periodic table…?

  -have outer electrons close to the nucleus so stronger attraction
• what did John dalton think atoms were?

  -solid spheres that couldn’t be divided
• what did JJ Thomson discover?

  -electrons

  -plum pudding model
• what did Ernest Rutherford do?

  -alpha scattering experiment

  -proved plum pudding was wrong

  -nuclear model
• what was the alpha scattering experiment?

  -positive alpha particles fired at a thin sheet of gold foil
• what is the nuclear model?

  -positive nucleus in centre where most mass is concentrated

  -Neil Bohr suggested electrons orbited nucleus in fixed shells
• how did Neil Bohr adapt the nuclear model?

  -electrons orbit nucleus in fixed shells
• what did later experiments discover?

  -protons

  -positive charge of a nucleus could be divided into smaller particles
• what did James Chadwick discover?

  -neutrons
• how did Rutherford disprove the plum pudding model?

  -his alpha scattering experiment

  -he expected alpha particles to pass straight through the gold foil or be slightly deflected however more particles were deflected than expected

  -so this suggested that atoms have a small nucleus where positive charge is concentrated
• how were elements arranged in the periodic table in the early 1800s?

  -atomic weight

  -physical and chemical properties
• what did Mendeleev adapt about the periodic table?

  -he left gaps

  -predicted new elements
• why did Mendeleev leave gaps?

  -for elements that he thought hadn’t been discovered
• what else did Mendeleev do as well as leaving gaps?

  -switched order of elements based on properties even if atomic weights were no longer in order
• how is the modern periodic table arrange?

  -atomic number

  -elements with similar properties in groups

  -metals on left

  -non metals on right
• why is it called the periodic table?

  -similar properties occur at regular intervals