The trends in ionisation energies across periods and down groups can be explained in terms of the atomic size, nuclear charge and the screening effect due to inner shell electrons.C4.1b explain how observed simple properties of Groups 1, 7 and 0 depend on the outer shell of electrons of the atoms and predict properties from given trends down the groups.C4 Predicting and identifying reactions and products.C2.3.2 explain how observed simple properties of Groups 1, 7 and 0 depend on the outer shell of electrons of the atoms and predict properties from given trends down the groups This is an extension of the periodic trend that the energy required to remove an electron increases going across a row of the periodic table.C2.3 How do metals and non-metals combine to form compounds?.6.13 Explain the relative reactivity of the halogens in terms of electronic configurations.6.5 Explain this pattern in reactivity in terms of electronic configurations.5.1 Atomic structure and the periodic table.Explain how the observed simple properties of Group 7 depend on the outer shell of electrons of the atoms and predict properties from given trends down the group.Explain how the observed simple properties of Group 1 depend on the outer shell of electrons of the atoms and predict properties from given trends down the group.Students should be able to: explain how properties of the elements in Group 1 depend on the outer shell of electrons of the atoms.Students should be able to: explain how properties of the elements in Group 7 depend on the outer shell of electrons of the atoms.4.1 Atomic structure and the periodic table.Explanations in terms of atomic radius, screening effect and nuclear charge for general trends in proprties of elements in groups I and VII.Explanations for general trends in values: (i) down a group Explanations for trends in values: (i) down a group The periodic table as a list of elements arranged so as to demonstrate trends in their physical and chemical properties.Unit C1: Structures, Trends, Chemical Reactions, Quantitative Chemistry and Analysis.1.6.20 demonstrate knowledge and understanding of how the reactivity down the group depends on the outer shell electrons of the atoms.1.6.14 demonstrate knowledge and understanding of how the trend in reactivity down the group depends on the outer shell electrons of the atoms.Unit 1: Structures, Trends, Chemical Reactions, Quantitative Chemistry and Analysis.1.2.13 explain the trend in the first ionisation energies of atoms down Groups and across Periods in terms of nuclear charge, distance of outermost electron from the nucleus, shielding and stability of filled and half-filled subshells.Unit AS 1: Basic Concepts in Physical and Inorganic Chemistry.RSC Yusuf Hamied Inspirational Science Programme.Introductory maths for higher education.
The physics of restoration and conservation.When they do react they produce hydroxides and hydrogen. The reactions of the elements with water become more vigorous down the group. For similar reasons the electronegativity decreases. This is because as the ions get larger the distance between the bonding electrons and the positive nucleus gets larger and reduces the overall attraction between the two. Generally the melting point of the alkali metals decreases down the group. There is more shielding between the nucleus and the outer electrons and the distance between the nucleus and the outer electron increases and therefore the force of attraction between the nucleus and outer most electrons is reduced. Going down the group, the first ionisation energy decreases. Progressing down group 1, the atomic radius increases due to the extra shell of electrons for each element. They are called s-block elements because their highest energy electrons appear in the s subshell. Group 1 elements are known as Alkali Metals. Note: Even though Hydrogen will appear above Lithium on the periodic table it is not considered a part of Group 1.
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