I know that the elements in group one have one electron in the outer shell and group twoelements have two in the outer shell. Answer Save. 4 years ago. It uses these reactions to explore the trend in reactivity in Group 1. Still have questions? ---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. To have a +1 charge there has to be one more proton than there is electron which isn't the case. In Group 1, lithium carbonate behaves in the same way - producing lithium oxide and carbon dioxide.. ; The transition metals are much harder, stronger and denser than the Group I metals, which are very soft and light. 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. A. All of the Group I metals form ions with a +1 charge while the transition metals can form ions with variable charges. For example, copper usually has a +1 or +2 valence, while iron typically has a +2 or +3 oxidation state. Hence, elements cannot lose electrons easily. As a result, the 2 ionization process needs much more energy than the 1st ionization process. 0 0. The effect of an increased atomic size is greater as compared to the increased nuclear charge. General Properties of the Alkali Metals. Learn term:family 1 = alkali metals, charge = +1 with free interactive flashcards. The following elements have only one possible charge, so it would be incorrect to put a Roman numeral after their name. Hence, Group 17 elements are strong non-metals, while Group 1 elements are strong metals. 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. Relevance. Join Yahoo Answers and get 100 points today. They include lithium (Li), sodium (Na) and potassium (K). this also means they lose electrons. a 1 : 1 ratio. 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. And why do those in group two have a 2+ charge etc. The elements have very similar properties: they are all shiny, silvery-white, somewhat reactive metals at standard temperature and pressure.. All of these metals react vigorously or even explosively with cold water. The densities of the Group 1 elements increase down the group (except for a downward fluctuation at potassium). Choose from 500 different sets of term:family 1 = alkali metals, charge = +1 flashcards on Quizlet. Metal ions may have other charges or oxidation states. As a result, the electronic configuration of the group 1 elements having +1 charge is the same as the inert gas. The key difference between group 1 metals and transition metals is that group 1 metals form colourless compounds, whereas transition metals form colourful compounds.. Group 1 metals are also known as alkali metals because these elements can form alkaline compounds. Ask question + 100. Most carbonates tend to decompose on heating to give the metal oxide and carbon dioxde. To illustrate, an atom of an alkali metal (group 1) loses one electron and forms a cation with a 1+ charge; an alkaline earth metal (group 2) loses two electrons and forms a cation with a 2+ charge, and so on. For example, all cations formed from sodium atoms have a +1 charge, so Na + is named sodium ion, without the Roman numeral for the charge. For example, a typical Group 2 carbonate like calcium carbonate decomposes like this:. The elements in Group 1 of the Periodic Table are called the alkali metals. So groups 2, 13-18 do not form ions with a 1+ charge. This group lies in the s block of the periodic table. These elements want to remove this single electron from their outer shell in order to return to a state with 8 valence electrons. Awesome. ; They have much higher melting points e.g. Group 1 elements are known as Alkali Metals. Group 1 metals all react with cold water, in some cases very violently indeed. 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) Group 1 metals C. Group 2 metals D. Group 3 metals E. Metalloid Since the charge on the group 1 metal ions is +1, and the charge on halide ions is -1, its easy to predict the formula of any ionic compound formed between an alkali metal and a halogen i.e. This page looks at the reactions of the Group 1 elements - lithium, sodium, potassium, rubidium and caesium - with water. Group 1 consists of: lithium, sodium, potassium, rubidium, caesium and francium and collectively known as the alkali metals. What is the charge on these ions? Hydrogen is usually placed at the top of the Group but is not a Group 1 metal. Group 2 include: beryllium, magnesium, calcium, strontium, barium and radium. Atomic and Ionic Radii of Group 1 and Group 2 elements : Typically, the atomic radius is measured as half of the distance between the nuclei of the two bonded atoms. They have lower effective nuclear charge when one moves left to right in a column. Physical Properties. The alkaline earth metals are six chemical elements in group 2 of the periodic table.They are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). The reaction produces hydrogen gas and the hydroxide of the metal, which is strongly alkaline, giving the group its alternative name, ... the group one metals end up as ions with one positive charge. 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 … They are highly reactive; Reactivity increases down the group – because tendency to loose one electron increases down the group due to increase increase in size and decrease in nuclear charge 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. Group 1 elements: Trend of change in the physical properties: The atomic radius (atomic size) of alkali metals increases gradually . In the main group elements, the s and p blocks (groups 1,2, 13-18), only the alkali metals (group 1) form ions with a charge of 1+. Transition metals B. 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