Topic 1.1- Key concepts Flashcards
Atomic structure, Periodic table
How has the dalton model changes over time?
- Dalton believed atoms couldn’t be broken down
- Plum Pudding: Thompsons experiments with cathode rays proved negatively charged electrons
-Nuclear model: Rutherford gold foil experiment discovered a positively charged nucleus and is mostly empty space
Why do atoms contain the same number of electrons and protons?
For it to have neutral charge
How much smaller is the nucleus of an atom compared to the size of the atom?
100,000 times smaller
What is the mass of a neutron and proton?
1
What is the mass of an electron?
1/1837
what does mass of an atom mean?
the sum of individual particles (neutrons and protons)
What is an isotope?
-Same electrons and protons
-Different number of neutrons
-Affects weight
What is the atomic number?
The number of protons
How is the periodic table organised?
Increasing atomic number
How to calculate relative atomic mass?
Total abundance
How big is an atom
0.1 nm radius
How did Mendeleev arranged the elements?
Rows by increasing atomic mass
How was Mendeleev able to predict the existence and properties of new substances?
- Noticed every eighth element had same properties as the first, made rows of seven
- Left gaps when atoms didn’t fit in a group
What was wrong about Mendeleev’s organisation?
Atomic mass didn’t take into account:
-Relative atomic mass
-Isotopes
What are the rows called? And what do these mean?
Periods, number of rings/orbitals.