Periodic table Flashcards
How did Mendeleev order the periodic table?
- Increasing atomic weight
- Which meant that there were gaps for undiscovered elements
- Showed elements with similar chemical properties lined up in groups
Why was Mendeleev’s periodic table accepted
predicted the properties of an element (gallium) which he left a gap for
What is an isotope?
An element with the same amount of protons and electrons but a different amount of Neutrons
How to calculate relative atomic mass of isotopes?
1) multiply atomic mass by the abundance
2) add the values from step one together
3) divide values from step two by total abundance
Properties of metals
- Solid at room temp
- High melting point
- Good conductors
- Shiny
- Hard and strong
- Form basic oxides
- Positive ions formed
- Malleable and ductile
Properties of non-metals
- solid, liquid and gas at room temp
- Low melting points
- Insulators except carbon
- Dull
- Brittle
- Form acidic oxides
- Form negative ions
Why do the group 1 elements get more reactive as you go down the group?
- Atom itself is bigger
- Outer shell electrons further away from the nucleus
- Attraction between outer shell electrons and nucleus is weaker
- electron can be lost more easily therefore element more reactive
Why do the boiling point of the noble gases increase as you go down?
- The mass increases as the atoms get bigger
Properties of the group 1 elements
- Lower melting points in comparison to other metals
- Low density
- High reactivity
- Soft
- Good conductors
Properties of the group 0 elements
- Unreactive
- Low boiling point
Reaction of lithium in water
- React with the oxygen to create a layer of oxide
- Floats on the water and gives off hydrogen gas
Reaction of sodium with water
- Reacts more quickly than lithium with oxygen
- Floats on water and gives off hydrogen gas more vigorously
- Melts into a ball
Reaction of potassium with water
- Reacts more quickly than sodium with oxygen
- Hydrogen gas reacts with the heat and catches fire
Why does the reactivity of the halogens decrease as you go down the group
- Atoms get bigger as they go down the group
- Smaller the atoms the greater the forces of attraction between the nucleus and outer shell electrons
- When they gain electron(s) in reaction, attraction between gained electron is weaker because of the size of the atom.