It uses these reactions to explore the trend in reactivity in Group 1. All the metals … Because beryllium's chemistry is so different from the other group 2 elements, the term "alkaline earth" is usually restricted to Mg, Ca, Sr, Ba, Ra. Group 1 elements: Trend of change in the physical properties: The atomic radius (atomic size) of alkali metals increases gradually . Group 1 elements have a valence of 1, meaning they have 1 outer shell electron. Group 1 metals all react with cold water, in some cases very violently indeed. This is a chart of the most common charges for atoms of the chemical elements. ---TRANSITON--- Transition and heavier elements have a more complex electron structure than (lighter) Representative elements ALL transition elements are metals and will lose electrons (oxidation) and obtain a positive ion charge Many transition elements may have more than one charge in their ionic form. Group I (alkali metals) carry a +1 charge, Group II (alkaline earths) carry a +2, Group VII (halogens) carry -1, and Group VIII (noble gases) carry a 0 charge. The charge of an ion of an element in group 1 (Li, Na, K, etc) is +1. The elements in Group 1 of the Periodic Table are called the alkali metals. 0 0. The Group 1 metals are all highly reactive silvery metals that are so reactive to air and moisture that they must be stored under an inert atmosphere or oil. Hence, Group 17 elements are strong non-metals, while Group 1 elements are strong metals. All Group 1 elements: (a) are soft, solid, shiny metals at room temperature and pressure that are good conductors of heat and electricity (b) have 1 valence electron (1 electron in the highest energy level) (c) are very reactive (d) form cations with a charge of +1 (M +) when they combine with non-metals in an ionic compound(e) form white ionic compounds (4) What is the charge on these ions? ; The transition metals are much harder, stronger and denser than the Group I metals, which are very soft and light. I know that the elements in group one have one electron in the outer shell and group twoelements have two in the outer shell. That means the electronic configuration is very stable and they does not want to lose another electron. Metals are very reactive with chemical reactivity increasing down the group. A. The result of this weaker bonding is a reduction in the melting point of the alkali metals on descending the group … Easy to cut; Shiny when freshly cut; Low density; Chemical Properties. For example, a typical Group 2 carbonate like calcium carbonate decomposes like this:. However, group 1 of the periodic table contains hydrogen, which is a nonmetal. Ask question + 100. All of these metals react vigorously or even explosively with cold water. Group 1 metals C. Group 2 metals D. Group 3 metals E. Metalloid The group 17 elements include fluorine(F), chlorine(Cl), bromine(Br), iodine(I) and astatine(At) from the top to the bottom. Group 2 include: beryllium, magnesium, calcium, strontium, barium and radium. In Group 1, lithium carbonate behaves in the same way - producing lithium oxide and carbon dioxide.. Another point mentioned in the book by Bahadur, under the chapter "s-Block Elements - The Alkali Metals", under Complex Ion Formation is that the Group 1 metals, i.e., the alkali earth metals have a larger size, low nuclear charge and hence don't tend to form complexes too easily. And why do those in group two have a 2+ charge etc. Join Yahoo Answers and get 100 points today. You can use this chart to predict whether or not an atom can bond with another atom.The charge on an atom is related to its valence electrons or oxidation state.An atom of an element is most stable when its outer electron shell is completely filled or half-filled. Still have questions? Group 1 ions have a charge +1 . For example, copper usually has a +1 or +2 valence, while iron typically has a +2 or +3 oxidation state. This group lies in the s block of the periodic table. this also means they lose electrons. The following elements have only one possible charge, so it would be incorrect to put a Roman numeral after their name. Various properties of the group 1 elements are summarized in Table 21.3 "Selected Properties of the Group 1 Elements". ; For example iron can form an Fe 2+ ion or an Fe 3+ ion. 1 Answer. The answer to your question is quite simple.The alkali metals of group 1 grow larger in size downwards and since the effective nuclear charge remains the same as we go down group 1 the number of shells also increases and so it is easy to lose an electron and therefore as we move downwards the reactivity … However, I thought charge depended on the number of protons and electrons. ; They have much higher melting points e.g. GROUP 1: Alkali Metals Physical Properties. Group (1 & 2) belong to the s-block of the Periodic Table. Answer Save. Atoms of many main-group metals lose enough electrons to leave them with the same number of electrons as an atom of the preceding noble gas. 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