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A hydrogen bond is the attractive interaction of a hydrogen atom covalently bonded to a very electronegative atom, such as nitrogen, oxygen or fluorine, to another very electronegative atom in another molecule.The interaction is essentially electrostatic between the small positive charge on the hydrogen atom and the slight negative charge on the N, O or F atom in the other molecule.Examples are the hydrogen bonding in liquid water, alcohols, ammonia and also in solids, ice, solid hydrogen fluoride.In larger molecules that have the right shape the hydrogen bonding can occur within the molecule between a hydrogen atom covalently bonded to a very electronegative atom, such as nitrogen, oxygen and a very electronegative atom in another part of the molecule.
Atoms become larger as we go down a column of the periodic table, and they becomes smaller as we go across a row of the table.
Yes, hydrogen diffuses faster than methane. The hydrogen molecule, H2, is the smallest of all molecules and it is considerably smaller than the methane molecule, CH4. Smaller molecules move faster, and therefore diffuse faster, at any given temperature, than larger molecules.
The nitride ion has a larger negative charge than the fluoride ion and a smaller positive charge in its nucleus, which means a greater repulsion within the electron shells and a lesser attraction to the nucleus.
Ammonia is a gas at room temperature which has an irritating odor. It is highly soluble in water, in other words 702 mL of ammonia can be dissolved in 1 mL of water. Inhaling larger doses of ammonia will be fatal.
Yes, nitrogen molecules are smaller than butane molecules. Nitrogen molecules consist of two nitrogen atoms, while butane molecules consist of four carbon and ten hydrogen atoms. Carbon atoms are slightly smaller than nitrogen atoms, but four of them are definitely larger than two nitrogen atoms, and of course, there are also the ten hydrogen atoms, and although hydrogen atoms are the smallest type of atom, if you have ten of them it does contribute to the size of the molecule. Further to this, the distance between bonds will be smaller in N2 as this is a triple bond because of 3 shared electrons each, whereas it is single bonds between the carbons, elongating the bonds between carbons
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A hydrogen bond is the attractive interaction of a hydrogen atom covalently bonded to a very electronegative atom, such as nitrogen, oxygen or fluorine, to another very electronegative atom in another molecule.The interaction is essentially electrostatic between the small positive charge on the hydrogen atom and the slight negative charge on the N, O or F atom in the other molecule.Examples are the hydrogen bonding in liquid water, alcohols, ammonia and also in solids, ice, solid hydrogen fluoride.In larger molecules that have the right shape the hydrogen bonding can occur within the molecule between a hydrogen atom covalently bonded to a very electronegative atom, such as nitrogen, oxygen and a very electronegative atom in another part of the molecule.
A single oxygen atom is smaller than a molecule.
Atoms become larger as we go down a column of the periodic table, and they becomes smaller as we go across a row of the table.
NITROGEN
Air particles are gas particles. Some gas particle are larger than others, and the nitrogen (N2) and oxygen (O2) that make up 99% of our atmosphere are rather large, which is why lighter gases, such as hydrogen (H2) and helium (He) rise.
Because larger stars burn their hydrogen faster than smaller ones.
The atmosphere on Neptune contains helium and hydrogen with some traces of water, methane and ammonia. The atmosphere is similar to the large planets of the Solar System, but has a larger proportion of ice.
Negative Numbers.
Water has stronger hydrogen bonding, but not stronger hydrogen bonds than HF, but it does have stronger hydrogen bonds than ammonia. There are two things that affect the intermolecular forces in these molecules: the strength of the H-bond itself, and the number of them that can be formed between neighboring molecules. The larger the difference in electronegativity of the H atom and the other atom (N, O, and F), the stronger the H-bond. Therefore the order is N < O < F. However, HF can only form one H-bond to one neighbor, while water can form two thus promoting more intermolecular interactions. Ammonia, while it has 3 N-H bonds, has far weaker H-bonds due to the lower electron density on the N-atom compared to the O-atom in water. .