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Periodicity

Periodicity - Periodic Table

QuestionAnswer
What is periodicity? It is the recurrence of elements with similar physical and chemical properties at regular intervals in the periodic table.
How are elements arranged in the periodic table? In increasing order of atomic number. Into rows and columns based on their structure and properties. All elements in a period have the same number of atomic orbitals occupied. All elements in a group have the same number of valence electrons.
What is the periodic table? It is a classification of all known elements arranged according to their physical and chemical properties.
Who were the four scientists who contributed to the development of the modern periodic table? Johann Dobereiner, John Newlands, Dmitri Mendeleev and Henry Moseley.
What are metalloids? Intermediates between metals and non-metals. These include boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te) and polonium (Po).
What is a group? It is a vertical column of elements.
What is a period? It is a horizontal row of elements.
Group I metals are called alkali metals
Group II metals are called alkaline earth metals
Group VII metals are called halogens
Group 0 ( or VIII) elements are called noble/ inert gases
Between groups II and III, ten groups of elements are located. These are called transition metals
What does IUPAC stand for? International Union of Pure and Applied Chemistry
All elements in group VIII (or 0) have full outermost (valence) electron shell / stable electronic configuration.
What determines the chemical properties of an element? The number of valence electrons they have.
Define 'ion'. An electrically charged particle formed when an atom loses or gains electrons. The atom becomes ionised.
What is the 'ease of ionization'? The ease with which atoms lose or gain valence electrons.
What is electronegativity? It is a measure of how strongly an atom attracts electrons.
What is the MOST electronegative element in the periodic table? Fluorine (F)
What is the LEAST electronegative element (most electropositive) in the periodic table? Francium (Fr)
What is the link between reactivity and ease of ionization? The easier it it for an atom to become ionized, the more reactive it will be.
What are the 3 main factors which affect the ease of ionization/reactivity of an atom? 1) Atomic radius - distance between nucleus and valence electrons. 2) Nuclear charge - the number of protons in the nucleus. 3) Shielding/screening - the number of electron shells between the nucleus and the valence shell.
What happens DOWN a group of metals with respect to atomic radius, electrostatic force of attraction and reactivity? - Atomic radius INCREASES due to greater shielding effect - Electrostatic force of attraction between nucleus and valence electrons DECREASES - Tendency of the atom to LOSE its valence electrons increases (i.e. ELECTROPOSITIVITY increases).
What happens UP a group of non-metals with respect to atomic radius, electrostatic force of attraction and reactivity? - Atomic radius DECREASES due to less shielding effect - Electrostatic force of attraction between nucleus and valence electrons INCREASES - Tendency of the atom to GAIN electrons from another atom increases (i.e. ELECTRONEGATIVITY increases)
What happens ACROSS a period from left to right with respect to atomic radius , electrostatic force of attraction and reactivity? Atomic radius DECREASES but shielding effect remains the same. Size of NUCLEUS increases due to increasing number of protons in the nucleus (nuclear force increases). Electrostatic force of attraction therefore increases. Electronegativity increases.
What is the shielding effect? This refers to the effect of atomic shells/orbitals between the nucleus and the electrons on the valence shell. The more shells there are, the weaker the electrostatic force of attraction between the nucleus and the valence electrons.
What is electropositivity? The tendency of metals to lose their valence electrons
What is ionization energy? The amount of energy required to remove an electron from an atom. The greater the amount of energy, the more difficult it is for that atom to lose electrons.
What is electron affinity? The degree to which an atom attracts electrons (super simplified definition - more advanced later).
Created by: Ms.Kumar
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