The Atom - Electronic Structure and Ionisation Energies Flashcards
What is the electronic configuration of argon?
State the block in the periodic table to which argon belongs. (2)
1s2 2s2 3p6 (1)
P (block) (1)
What is meant by the term ‘first ionisation energy’? (2)
Enthalpy change when an electron is removed (1) from a GASEOUS atom (1)
Write an equation to illustrate the process occurring when the SECOND ionisation energy of sodium is measured. (2)
Na+(g) –> Na2+(g) + e-
Equation (1) State Symbols (1)
What affects the attraction of an electron to an atom? (3)
It’s distance from the nucleus (1)
(Electron) shielding (1)
Nuclear charge (1)
How many electrons are in the s sub level and how many orbitals does it have? (1)
2 electrons AND 1 orbital (1)
How many electrons are in the p sub level and how many orbitals does it have? (1)
6 electrons AND 3 orbitals (1)
How many electrons are in the d sub level and how many orbitals does it have? (1)
10 electrons AND 5 orbitals (1)
What is the relative charge and mass of a proton? (1)
Relative mass = 1 AND charge = +1 (1)
What is the relative charge and mass of a neutron? (1)
Relative mass = 1 AND relative charge = 0 (1)
What is the relative charge and mass of an electron? (1)
Relative mass = negligible AND relative charge = -1 (1)
What are the four main stages Involved in obtaining the mass spectrum of a sample of gaseous atoms? 4)
Ionisation (1)
Acceleration (1)
Deflection (1)
Detection (1)
Define the term ‘relative atomic mass’. (2)
The average (1) mass of an atom
——————————————– x12
The mass of an atom of 12C (1)
Define the term ‘relative molecular mass’. (2)
The average (1) mass of 1 mole of a molecule
—————————————————————- x12
The mass of one mole of 12C (1)
What affects how much the ion is deflected during the deflection stage of the mass spectrum? (2)
It’s mass (1)
It’s charge (1)
How do we alter it so the heavier ions are detected? (1)
Alter the strength of the magnetic field (1)
