Melting points increase with atomic weight for elemental halogens (the second-most right column in a Periodic Table). The heavier the atom, the harder to turn it into a liquid.
The lightest halogens, such as Florine (F) and Chlorine (Cl) are gasses at room temperature, having "melted" and "boiled" at lower (colder) temperatures.
The two heaviest halogens are Iodine (I) and Astatine (At). Astatine is very rare, but Iodine is common and is a solid at room temperature. The have the highest melting points of halogens.
Remember, F down to At increase in melting points.
F and Cl are gases, so they have low melting point.
Br is a liquid, so it has a higher melting point.
I and At are solids so it takes more heat to melt them.
all group 2 metals are light weight with high melting points beryllium however has the highest melting point due to the low number of electrons shielding the nucleus fro the delocalised atoms
1.Brittleness 2.High Melting Points 3.High Boiling Points
if this is from castlelearning its choices 1. H2O(s) 2. Na2O(s) 3. SO2(s) 4. CO2(s) the answer is choice 2 because sodium, Na, is a metal. When a metal is bonded to a nonmetal such as oxygen, an ionic bond is formed. Ionic compounds have high melting points. All of the other are nonmetal which mean they are convalent compounds and covalent compounds have low melting points. JgLy<3 :)
1)high melting and boiling points 2)solubility 3)Electrolytes
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all group 2 metals are light weight with high melting points beryllium however has the highest melting point due to the low number of electrons shielding the nucleus fro the delocalised atoms
1. Alkali metals are soft and highly reactive. 2. They have low melting points and densities.
The melting point of copper is 1084,62 0C and the boiling point is 2 562 0C.
1.Brittleness 2.High Melting Points 3.High Boiling Points
you play to 25 points but have to win by 2 points
1)brittleness 2)high melting points 3)high boiling points
Melting points are very different.
if this is from castlelearning its choices 1. H2O(s) 2. Na2O(s) 3. SO2(s) 4. CO2(s) the answer is choice 2 because sodium, Na, is a metal. When a metal is bonded to a nonmetal such as oxygen, an ionic bond is formed. Ionic compounds have high melting points. All of the other are nonmetal which mean they are convalent compounds and covalent compounds have low melting points. JgLy<3 :)
Molybdenum with 2 623 0C.
1)high melting and boiling points 2)solubility 3)Electrolytes
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Group VII elements are halogens. Halogens exist as diatomic covalent molecules (the 2 atoms within each molecule are held together by strong covalent bond) and they are very reactive non-metals. Physical properties: On going down the group from Fluorine to Astatine, - the melting and boiling points of the halogens increase. Chlorine is a gas, bromine is a liquid and iodine is a solid at room temperature. - the colour of the halogens become darker. Chlorine is greenish-yellow, bromine is reddish-brown and iodine is purplish-black. Chemical properties: - Halogens react with most metals to form salts called halides. - The reactivity of halogens decreases down the group. Fluorine is the most reactive. This is because the atomic size of the halogens increases down the group. It becomes more difficult for the nucleus to attract an electron into the valence shell to become an ion. - A more reactive halogen will displace a less reactive halogen from an aqueous solution.