why does ammonia exist in liquid state while other hydrides of 5th A group elements exists in other state.?
444782
Phosphine, arsine, and ammonia are all gases at ambient temperature and pressure.  But ammonia has a higher boiling point than the other 2, about -33 C.  All 3 are polar molecules.  But ammonia can form hydrogen bonds.  This increases the strength of the intermolecular forces, causing the liquid state to be more stable.
556249
In Be and Mg only the s subshell is full while the p is completely vacant. Moreover for every element the most stable state is tht of the nearest noble gas configuration. So for Be and Mg it will be quite easy to give to 2 electrons to get the nearest noble gas configuration to make stable cations. Hence they are not inactive/inert. Also they can gain electron pairs in the p-subshell (although it is energetically not favourable) so they can not be inert.
541563
Hydrogen is generally accepted as a member of group I or IA, but it is also accepted as having no group.  Allow me to explain.  \n\nHydrogen can be classified as a member of group I because like all of the other elements in group I, it has exactly one valence electron (one electron on its outermost electron shell, in the case of hydrogen, the only shell). Valence shell counts and electron configurations are the basis of the periodic table. \n\nHowever, hydrogen is very unique and exhibits far different chemical properties from any other element in group I or any other group.  For example, hydrogen is a non-metal, it exists in a diatomic state in nature, it can form compounds with both metals and non-metals, and does not form salt compounds with non-metals. For these reasons, sometimes periodic tables will not have hydrogen in group I.  Instead, some periodic tables will put hydrogen in a small box by itself above the rest of the periodic table, totally separated from the rest of the periodic table.  The little box for hydrogen in these periodic talbes is usually pretty close to the middle to represent the fact that it exhibits properties on both sides of the periodic table.  \n\nIn conclusion, either "no group" or group I or IA is acceptable to answer the homework question.
247481
If I'm not mistaken, they will have the same pressure, as they are in equal number of molecules. 17grams of Amonia or NH3 sum up 1mol of NH3 molecules while 2 grams of Hydrogen, H2 consists of 1mol of Hydrogen molecules. \nAn equation : Pv = nrT, where P= pressure, v=volume, n is the number of molecule/atom, r is a constant, and T is the absolute temperature (in Kelvin). Since they are equal in their number of molecules, it share the same pressure. Hope it helps.
549677
This is a chemistry question, the anomaly is due to Hydrogen bonding.
592234
3g of hidrogen (plus 14 g of nitrogen) make up 17g of ammonia (H+H+H+N=1+1+1+14), so:\n\n3g  H____17g NH3\n50g H____=283.33g NH3\n\nI assumed a 100% efficient reaction (that means every bit of reactant will actually react).
438289
Co(NH3)4 would be more likely
20570
Mercury is a liquid at room temperature but can be changed to a solid if cooled to a low enough temperature or changed to a gas if heated to a high enough temperature.  This is similar to ice, water and steam but at different temperatures.\n\nIf we start with ice kept well below freezing, we can add heat and the ice will rise to the freezing point of water then begin to melt.  Melting occurs because we are adding heat energy to the water molecules which makes them vibrate.  At some point the vibrations are strong enough to break the attractive bonds between the frozen water moleclues which then become liquid.  When the ice is all melted we can add more heat to the water to raise its temperature to the boiling point.  At the boiling point the water molecules are vibrating strongly enough that some of them escape from the surface of the water to form a vapor or steam.  As more heat is added, more molecules escape and the water evaporates.\n\nMany materials, including mercury, exhibit similar solid, liquid and gaseous states depending on the temperature and strength of bonds.
468805
in water: a molecule of water will hyrdoyse the iron ion creating an iron hydroxide ion and a hydronium ion.  If the water is evaporate you still have the same compound except with some water trapped in the crystal structure.\n\nin ammonia: a co ordination complex is formed using 6 ammonia ligands [Fe(NH3)6]NO2\n\nAnd i don't actually know what would happen in hyrochloric acid
419911
That's easy. [Co(NH3)6]Cl3. This is coordination chemistry, dude. There can be other products depending on the ammonia concentration. But this is your best bet. I've been doing these reaction in the lab way way back.
761517
ammonia, NH3, dissolves in water by forming the ammonium ion.\n\nNH3+H2O--> NH4+ + OH-\n\nthe ammonia gains a proton from the water\na proton is hydrogen(atomic number 1=1 proton)
957050
all things have a solid liquid and gas state. it just depends on the temperature.
1080354
NaCl IS A MOLECULE CALLED TABLE SALT!\nNH3 is not a molecule because the nitrogen atom is not bonded to another atom/atoms using all of its valence electrons and is therefore not a molecule, it is an ion.
487836
mercury is one of five elements that are liquid at or near standard room temperature (the others are the metals caesium, francium, and gallium, and the nonmetal bromine). ...
839277
Flaw in problem statement: hydrogen azide is HN3 -- NH3 is ammonia.  As usual, you will need the molar concentrations.  if the salts fully dissociate, the hydrogen from the HN3 will be added to the hydrogen in the water, and you can add these up to get the total hydrogen present.  From that, you can get the pH.
228883
One of the things which effects the boiling points of substances is the intermolecular forces of attraction between the particles....the higher thr attractive forces, the higher the boiling point.\n\nWhich molecule has the higher attractive forces, Methane (Ch4) or Ammonia (NH3)?\n\nSince Methane is a small, nonpolar, hydrocarbon, the only attractive force its molecules experience is london forces (AKA induced dipoles).\nAmmonia on the other hand not only experiences london forces, but also experiences one of the most attractive forces...Hydrogen bonding.  The Hydrogens on the ammonia molecule are held in a polar bond with the Nitrogen making them form a partial positive charge and the Nitrogen forms a partial negative charge.  When the partial + Hydrogens from other NH3 molecules get near the parial - Nitrogens, they are attrcted to eachother which raises the boiling point of the substance.\nFor this reason, Ammonia gas will have a higher boiling point than methane.  This is confirmed by looking at the actual boiling points for each gas.\n\nBOILING POINTS:\nAmmonia: -33.5 degrees C\nMethane: -161.6 degrees C
806618
The only difference I can see would be the molecular geometry, due to the number of H's bonded onto the anion. Also, when drawing the Lewis dot structures, NH3 (N) would have one lone pair of electrons, HF (F) and H2O (O) would have two. This would dictate their structures according to the VSEPR rules.