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.C2.3 How do metals and non-metals combine to form compounds? The reactivity series of metals is a list of metals arranged in their order of reactivity from highest to lowest.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. Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n 4 and the atom emits a photon of light.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.While these are the most common valences, the real behavior of electrons is less simple. 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. You may assume that the valences of the elementsthe number of electrons with which an atom will bond or formare those that can be derived by looking at the groups (columns) of the periodic table.The Group 1 metals become more reactive towards water as you go down the Group. Caesium hydroxide and hydrogen are formed. Caesium explodes on contact with water, quite possibly shattering the container. Unit 1: Structures, Trends, Chemical Reactions, Quantitative Chemistry and Analysis Rubidium hydroxide solution and hydrogen are formed.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. ![]() Rubidium is an element with atomic symbol Rb, atomic number 37, and atomic weight 85.468. Which is less reactive: lithium (Li) or beryllium (Be) Answer. So by reactivity series you can tell which metal will displace another. Shipped in very limited quantities sealed in a copper tube and over packed in a wooden box. Answer: Rubidium (Rb) is more reactive because it is further to the left than strontium (Sr). The alkali metals include: lithium sodium potassium rubidium cesium and francium.
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