C1 Flashcards
How did JJ Thompson discover the electron?
- experimented with a cathode ray tube
- the beam moved towards the positively charged plate, so he knew the particles must be negative
What are the three ideas Dalton had about the atom?
- cannot be created or destroyed
- all atoms of the same element are the same
- they join, to make new substances
Describe Rutherford model of the atom
- mass is concentrated in centre
- mostly empty space
- electrons travel in random paths
What is the radius of a nucleus, and how does it compare to the actual radius?
- nucleus radius = 1X10⁻¹⁴m
- it is 1/10000 of the atomic radius
How did Mendeleev arrange the periodic table?
- elements arranged in order of increasing atomic mass
- elements with similar properties put in groups
- switched positions of some elements
- gaps left for undiscovered elements
Why did Mendeleev’s table lack accuracy?
- isotopes were understood poorly
- protons and neutrons had not been discovered
How are elements arranged in the modern periodic table?
Increasing atomic number
What determines whether an element is a metal or non-metal?
The atomic structure they have
What does it mean if the ionic compound ends in -ide?
The compound has 2 elements
What does it mean if an ionic compound ends in -ate?
Compound contains three elements at least, including oxygen
Describe the structure of an ionic compound
- lattice structure
- regular arrangements of ions
- ions held together by strong electrostatic forces between ions of opposite charge
- conduct when aqueous or molten, as charged particles are free to move
Describe the structure of simple molecular compounds
- have weak intermolecular forces, but throng covalent bonds (low melting and boiling points)
- do not conduct as they are not charged particles
What are the uses of graphite?
- electrodes (conducts and has a high melting point)
- lubricant (slippery)
What is a fullerene?
A molecule made of carbon, shapes like a closed tube or hollow ball
What are the properties of buckminsterfullerene (C₆₀)?
- slippery (weak intermolecular forces)
- low melting point
- strong covalent bonds between carbon
- large surface area