Free QCE Year 11 Chemistry Flashcard Review
Review 20 public cards with spaced repetition. Flip a card, then grade your recall. Cards you miss return today. Your schedule stays in this browser.
Loading your review schedule…
Browse the free cards
What three particles make up an atom and their charges?
Proton +1, neutron 0 (both in nucleus), electron −1 (outside nucleus).
How many neutrons in ³⁷₁₇Cl?
37 − 17 = 20 neutrons.
Why do isotopes have the same chemical properties?
They have the same number of electrons and the same electron configuration.
Define relative atomic mass.
Weighted average mass of the naturally occurring isotopes relative to 1/12 the mass of a carbon-12 atom.
Order of subshell filling to Z = 36?
1s 2s 2p 3s 3p 4s 3d 4p.
Electron configuration of Cr?
[Ar] 3d⁵ 4s¹ (half-filled d subshell is extra stable).
Configuration of Fe³⁺?
[Ar] 3d⁵ — the 4s electrons are lost first.
What does a big jump in successive ionisation energies indicate?
The next electron is removed from an inner shell; electrons before the jump are valence electrons.
Why do hydrogen emission lines converge?
Energy levels get closer together further from the nucleus, so the gaps (and line spacing) shrink at higher energy.
What does AAS measure and how is concentration found?
Absorbance of a metal's characteristic wavelength; concentration is read from a calibration curve of standards.
Trend in first ionisation energy across period 3?
Generally increases, because core charge increases while the shell number stays the same.
Nature of period 3 oxides from Na to S?
Basic (Na₂O, MgO), amphoteric (Al₂O₃), then acidic (SiO₂, P₄O₁₀, SO₃).
What is a pure substance?
Matter with a fixed composition and constant properties; either an element or a compound.
Element vs compound?
An element has one kind of atom; a compound has two or more elements chemically bonded in a fixed ratio.
Homogeneous mixture?
Uniform composition with one visible phase, e.g. salt water, air, brass.
Heterogeneous mixture?
Non-uniform composition with visibly distinct regions, e.g. sand in water.
How does an impurity affect melting point?
It lowers the melting point and makes it melt over a range rather than sharply.
Why are ionic solids brittle?
A shift brings like-charged ions together; repulsion splits the crystal.
Why do ionic compounds conduct only when molten or dissolved?
Ions become free to move and carry charge; in the solid they are fixed.
Model of metallic bonding?
A lattice of cations in a sea of delocalised electrons, attracted non-directionally.