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Alkali metals GIVE electrons (the only one electron that they do have) so that they may become balanced.
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Do metals take or give electrons when they are combined with other elements?
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What charge does an ion of an alkali metal have?
Your Alkali Metals are those elements on the leftmost column of the periodic table (except for Hydrogen). Lithium (Li), Sodium (Na), Potassium (K), Rubidium, Cesium, Francium. You can remember them as those that form the Alkali bases, Sodium Hydroxide (NaOH), and Potassium Hydroxide (KOH) among others. In Pure Metallic form, they would have a neutral charge. However, they are frequently found in ionic form where they loose an electron to form a positive ion with a +1 charge. Li+ Na+ K+ etc.
Why is an alkali metal so reactive?
Bohr's model of the atom explains the reactivity of group 1 metals, as it applies the rule that electrons are in fixed orbits, and that the shells fill up from the centre. If each shell is full it can't take any more electrons so for an electron to migrate into an already full shell another electron must take its place. This means that there will always be one electron on the outside until it undergoes ionic bonding with a non-metal and becomes a stable positive ion.
Do the halogens react with the alkali metals why or why not?
The electron configuration is why they react. The Alkali metals have one electron in their outer shell and to complete their outer shell need 7 more electrons. They can give, take or share electrons with other atoms. This is when the Halogens come in handy. The Halogens have 7 electrons in their outer shells, and need one more to complete the outer shell. These can react very easily because they have both the perfect amounts to fill their outer shells and become compounds. Other atoms with other amounts to become atoms not ions needs another element to react with. Hope this helps, Matt.
What type of bonding happens to metalloids and metals and why?
• Metalloids: usually form covalent bonds with atoms of metals, nonmetals and other metalloids. They can easily take electrons from metals and lose electrons to nonmetals. • Metalloids: usually form covalent bonds with atoms of metals, nonmetals and other metalloids. They can easily take electrons from metals and lose electrons to nonmetals. They form because they want their valence shell to be full. Metals usually lose valence electrons because they want to stabilize their valence shell. Metalloids depends because they have different properties of metals and non metals.
Do metals take electrons or give electrons to the atoms they bond with?
Metals give up electrons while non-metals gain electrons
The ability of metals to give-off and take-in electrons thus producing a current?
conductivity
What is the bonding process for nonmetals bonding with metals?
the bonding process for nonmetals bonding with metals is that they can take electrons and give them to each other.
Do metals take or give electrons when they are combined with other elements?
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Why do halogens react so easily with Alkali Metals?
The electron configuration is why they react. The Alkali metals have one electron in their outer shell and to complete their outer shell need 7 more electrons. They can give, take or share electrons with other atoms. This is when the Halogens come in handy. The Halogens have 7 electrons in their outer shells, and need one more to complete the outer shell. These can react very easily because they have both the perfect amounts to fill their outer shells and become compounds. Other atoms with other amounts to become atoms not ions needs another element to react with. Hope this helps, Matt.
What charge does an ion of an alkali metal have?
Your Alkali Metals are those elements on the leftmost column of the periodic table (except for Hydrogen). Lithium (Li), Sodium (Na), Potassium (K), Rubidium, Cesium, Francium. You can remember them as those that form the Alkali bases, Sodium Hydroxide (NaOH), and Potassium Hydroxide (KOH) among others. In Pure Metallic form, they would have a neutral charge. However, they are frequently found in ionic form where they loose an electron to form a positive ion with a +1 charge. Li+ Na+ K+ etc.
Why is an alkali metal so reactive?
Bohr's model of the atom explains the reactivity of group 1 metals, as it applies the rule that electrons are in fixed orbits, and that the shells fill up from the centre. If each shell is full it can't take any more electrons so for an electron to migrate into an already full shell another electron must take its place. This means that there will always be one electron on the outside until it undergoes ionic bonding with a non-metal and becomes a stable positive ion.
Do metals lose or gain electrons in a chemical reaction?
Metals will lose electrons, most of the time. If you look at the first group on the periodic table, you will notice that these metals have one valence electron (Li, Na, K etc.). These are known to readily form ionic bonds with the halogens. For example Na and Cl form salt NaCl because the Cl strips the Na of it's valence electron leaving Na with a positive charge and Cl with a negative charge. Because of the differences in charges, they attract each other and form an ionic bond.
Do the halogens react with the alkali metals why or why not?
The electron configuration is why they react. The Alkali metals have one electron in their outer shell and to complete their outer shell need 7 more electrons. They can give, take or share electrons with other atoms. This is when the Halogens come in handy. The Halogens have 7 electrons in their outer shells, and need one more to complete the outer shell. These can react very easily because they have both the perfect amounts to fill their outer shells and become compounds. Other atoms with other amounts to become atoms not ions needs another element to react with. Hope this helps, Matt.
What type of bonding happens to metalloids and metals and why?
• Metalloids: usually form covalent bonds with atoms of metals, nonmetals and other metalloids. They can easily take electrons from metals and lose electrons to nonmetals. • Metalloids: usually form covalent bonds with atoms of metals, nonmetals and other metalloids. They can easily take electrons from metals and lose electrons to nonmetals. They form because they want their valence shell to be full. Metals usually lose valence electrons because they want to stabilize their valence shell. Metalloids depends because they have different properties of metals and non metals.
Why do the alkali metals react more violently as you go down the column in the periodic table?
Electron screening is the best reason for there being more reactivity as an investigator looks down the Group 1 elements, which are the Alkali metals. Let's take a step back and then come up to speed on this one. When any of the alkali metals react with water, they form a metal hydroxide, and that Group 1 element becomes the positive ion of that metal. The general reaction for any of the Alkali metals is this, where "M" is any metal: M + 2H2O --> M+ + 2OH- + H2.For all the Group 1 elements, those Alkali metals, it is this same reaction. In going down the column, the elements' atomic numbers increase, and there are more and more electron shells in the atomic structure. The increasing number of electrons sets up a condition where the outer electrons are "screened" from the positive "pull" of the nucleus by other electrons in inner shells. These outer electrons can be "shed" or "loaned out" more easily if the nucleus isn't "hanging onto them" as tightly. Electronegativities speak to the "desire" of an element to react, and we see electronegativities decreasing as we go down the column. The further down the column you go, the more violently they react because the electronegativity of the atoms decreases down the column. Because the electronegativity is decreasing (and that is because of the increasing size of the outer electron orbitals and the screening of those outer orbitals by inner electrons), the electrons are more easily removed from the metal. That means that it is easier to form the ion, and said another way, they are more easily oxidized. That means that less energy is spent in the reaction pulling off the electron, and so the reaction is faster and more exothermic.
What type of element tends to lose electrons when bonds form?
Metals because metals are mostly on the left side of the Periodic Table and have fewer electrons.
