Experiments
What experiment did J.J. Thompson use to discover the electron?
William Crooke's Cathode Ray Tube
What did Aristotle believe matter was made out of?
Fire, Water, Air, and Earth
Who created the periodic table? Describe how the elements were arranged back then compared to now.
The periodic table was created by Dmitri Mendeleev, and he arranged the elements by their chemical properties and atomic masses. Today, the periodic table is arranged by their chemical properties and atomic number.
Name 3 properties of a non-metal.
Brittle/Poor conductor of heat/Poor conductor of electricity/Dull lustre/Variations in colour/Ranges of states at room temperature/Opaque to transparent/Form anions
What is an orbital?
An orbital is a place/shape/area where an electron exists 90% of the time.
During the gold foil experiment, Ernest Rutherford was shocked to see what?
Who created the mathematical equations for the movement of electrons?
Erwin Shrodinger
Electroconductivity: An atom's ability to conduct electricity.
How many valence electrons do Alkali Earth Metals have?
2 valence electrons
Name the 4 quantum numbers.
1. Principle Quantum Number
2. Angular Momentum
3. Magnetic Quantum Number
4. Spin Number
Who hypothesised that electrons behaved like waves?
BONUS: Who later proved this theory?
Louis de Broglie
BONUS: Thomas Young
Name the person who came up with the Plum Pudding Model and describe what it is. (atom's appearance)
J.J. Thompson. The Plum Pudding Model was a theory where the atoms had a positive dough and a negative plums (electrons).
Describe the 3 factors that affect the size of an atom (atomic radii).
Number of Shells, Nuclear Charge, Electron Shielding
Name all of the families in the periodic table. (9)
Main (6)
Bonus (3)
Alkali Metals, Alkali Earth Metals, Transition Metals, Halogens, Noble Gases, Hydrogen
Bonus: Lanthanides, Actinides, Post-Transition Metals
What order of letters must you subtract when writing out cations in core notation?
p, s, d
What experiment did James Chadwick use to find the neutron?
He used Irene Joliot-Curie and her husband's beam created by hitting beryllium with alpha particles.
He found that the beam had the same mass as a proton, but wasn't affected by the charged plates or magnets.
Name all the people who contributed to the atomic theory history in order. (10)
Democritus, Aristotle, John Dalton, J.J. Thompson, Hantaro Nagaoka, Ernest Rutherford, Niels Bohr, Louis de Broglie, Erwin Shrodinger, James Chadwick
Describe what electronegativity is and how it affects families and periods the further you go along them.
Down: EN is decreased because of electron shielding
Across: EN is increased because nucleus has more protons (greater attraction)
Rank the following families by most reactive to least reactive:
Noble gases, Alkali earth metals, Halogens, Alkali metals
Alkali metals/Halogens, Alkali earth metals, Noble gases
Describe the orbital shape of d and f.
d: 4 teardrops/butterfly/weird pacifier
f: 6-8 ovals/crazy shapes
Explain how Niels Bohr discovered that there were multiple orbits.
1. Electricity gives energy to electron
2. Electron moves up an orbit
3. Electron loses energy and moves back down
4. Energy is released as photonic light (specific colour)
Different colours were produced from different elements; therefore having different orbitals.
Name and describe the 3 laws that were established by the time John Dalton made his new theory.
- Law of Conservation of Mass: Mass stays the same within a closed system
- Law of Definite Composition: Reactants combine in specific ratios
- Law of Multiple Proportions: Reactants can combine in different ways
What does it mean when a compound has a small inequality?
- Unequal sharing
- Polar covalent bond
- Electrons want to go towards atom with a higher electronegativity, and will spend more time there
Name 3 properties of Halogens.
F-At/Ions gain 1 electron/p5 have 7 valence electrons/All states of matter/Diatomic elements (bond in pairs)
Describe each of the 4 quantum numbers.
(1: Principle Quantum Number, 2: Angular Momentum, 3: Magnetic Quantum Number, 4: Spin Number)
1: Size/distance from the nucleus
2: Shape of the orbital
3: Orientation in 3D
4: Determines which electron goes up and down