Unit 1 A2 Production and uses of substances in relation to properties Flashcards
What are the elements in Periods 1, 2, 3, and 4 of the periodic table?
Period 1: Hydrogen, Helium. Period 2: Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, Fluorine, Neon. Period 3: Sodium, Magnesium, Aluminum, Silicon, Phosphorus, Sulfur, Chlorine, Argon. Period 4: Potassium, Calcium, Scandium, Titanium, Vanadium, Chromium, Manganese, Iron, Cobalt, Nickel, Copper, Zinc, Gallium, Germanium, Arsenic, Selenium, Bromine, Krypton.
What is the difference between s, p, and d blocks in the periodic table?
The s-block contains elements in Groups 1 and 2 (and helium), the p-block contains elements in Groups 13-18, and the d-block contains transition metals found in Groups 3-12.
How is the periodic table layout related to s, p, and d notation?
The periodic table is arranged into blocks (s, p, d) corresponding to the highest energy sublevel that is being filled in the elements’ electronic configuration.
How do you represent the electronic arrangement of elements using s, p, d notation?
Elements are represented by their electron configuration in terms of orbitals: 1s², 2s² 2p⁶, 3s² 3p⁶, etc., where s, p, and d denote types of orbitals.
What is first ionisation energy?
The first ionisation energy is the energy required to remove one mole of electrons from one mole of atoms in the gaseous state to form positive ions.
Why does ionisation energy increase across Period 2 to 4?
Ionisation energy increases across a period because the atomic radius decreases and the nuclear charge increases, making it harder to remove electrons.
Why does ionisation energy decrease down Groups 1, 2, and 7?
Ionisation energy decreases down a group because the atomic radius increases and the outer electrons are further from the nucleus, so they are more easily removed.
What is electron affinity?
Electron affinity is the energy change when an electron is added to a neutral atom in the gaseous state, forming a negative ion.
What is the trend of atomic radius across periods and down groups?
Atomic radius decreases across a period due to increased nuclear charge, and it increases down a group due to additional electron shells.
How does ionic radius change compared to atomic radius?
Ionic radius is smaller for cations (positive ions) and larger for anions (negative ions) than their corresponding atomic radii.
