keep in mind the role of binding energy
127369
The assembled nucleus has less energy than the collective nucleons. If it did not\n\na) it would not hold together with the collection of + charged protons, and\n\nb) it would not require added energy in the form of colliding particles to make it come apart.
618258
a the number of outer electron that will bond with other atoms to fill thei valence shells
123724
reactants...catalysts help a reaction by speeding it up (usually)...products are the end result of reactions...protons just aren't the right answer
368776
Atomic radius generally goes down as you go from left to right along any period of the Periodic Table.\nThis is due to the fact that more protons are being added to the nucleus, but the electrons are being added to the outer level in each case, and there is little or no extra shielding, so the forces of attraction get greater.\nThe only exception is the Transition Metals, where radius stays more or less constant.
131976
Because the bonds between the atoms are very strong, it takes a lot of energy to break them.
5714
Interesting scenario first of all i would like to comment. Well actually the bond is due to electronic forces. Hence mass has litle effect on the bond strength. Thus i thikn the effect of mass change should be a small one!! unless you change the charge of proton too!!
536362
It's good to see people actually thinking about what the terms they're using mean, rather than just plugging them into equations.\n\nBasically, the place where you seem to be confused is here:\n\n"In gas such as water vapour, intermolecular forces of attraction is weak and hence it has low PE"\n\nActually, this means the exact opposite, that the system has very high potential energy. Think about gravity for a minute - if a rock placed at, say, 1 foot above the ground were to fall to Earth, it would not release very much energy. Conversely, if the rock were placed 1 mile above the Earth, it would release a considerable amount of energy. The higher the rock is, the greater it's potential energy. However, the further the rock is away from Earth, the weaker the force of gravity acting on it - thus weak gravitational attraction corresponds to higher potential energy. Similarly with the particles in a gas - if they were to "fall" into a partially bound state such as that of a liquid, they would release energy, and thus the unbound state where the particles are too far away from each other to form bonds is the higher energy state.\n\nThis is not to say that a weaker force always corresponds to a higher energy state - if the reason that the force is weaker is that there is less mass/charge/whatever producing it, that really will lower the potential energy. But in the transition from a liquid to a gas does not change the charge of any of the particles - the reduction in intermolecular forces comes from the fact that the particles are moving out of each other's electrical potential wells, a process which, just like lifting up a rock, raises the potential energy.
356369
6.  The activation energy is the energy your system needs to acquire for a a successful chemical reaction to occur.  All reactions have an activation energy, whether it is positive or negative.  Heat needs adding to the reaction to introduce this energy, and even then it may only promote the reaction very slowly due to reactivity.  By introducing a catalyst you give the reaction an alternative pathway to go through which requires less energy because a more reactive intermediate is generated more quickly.  By introducing energy also your molecules move a lot more quickly and the likelihood of your two reactants colliding into each other to react is increased.\n\n7.  A catalyst promotes a reaction and helps it proceed at a faster speed than if this additive was not present.  An inhibitor prevents a reaction from occuring.  These are sometimes added to prevent oxidation processes.\n\n8.  A catalyst will increase the rate of a chemical reaction.  It does this by providing an alternative lower energy route to the product.  This lowers the activation energy.\n\nThere are some recent questions on catalysts which have been answered here, it may be worth doing a quick search as more in depth answers have been given previously.
465961
B\n\nStrong bonds requires more energy to break and therefore releases more energy when formed.\n\nSo when enthalpy(heat) is lowered you need something that eats more energy than it creates.
220374
Every living cell performs continuously thousands of different chemical reactions. Taken nutrients are transformed into a multitude of cell specific components. In this way, sugars, amino acids and their precursors, organic acids, nucleotides, lipids and other substances are produced. The totality of these reactions is summarized as the cell metabolism. In every chemical reaction, a bond is either formed or broken. This process does generally consume energy, consequently, the cell's metabolism and its energy balance to have be regarded as interdependent parameters. Every covalent bond of a molecule contains energy that is set free upon breaking down and that can subsequently be used for other purposes. It could, for example, be used for the formation of a new bond or it could be transformed into another form of energy like movement, warmth, light or electrical energy. Most chemical bonds and nearly all that occur within a cell are stable under physiological conditions. Hence, activation energy is needed for the break-down of a molecule. In chemical laboratories, high temperatures, high pressures or certain inorganic or organic catalysts are normally used. \n\nThe term activation energy refers to the minimum amount of energy required for a chemical reaction to occur. Most reactions require that atoms and molecules crash into each other with a great deal of force. These violent collisions must occur with enough energy to cause the chemical bonds within the molecules to be weakened or broken. When this occurs, the reactant molecules form an activated complex from which the product molecules are formed. Depending on the strength of the bonds within the reactant molecules the activation energy can be quite large, making the activated complex difficult to form.
249095
a) 1\n2) depends on if the outer shell is full or not. If it's full, they probably bounce off of each other, if not full, they can create a bond with each other.\n3) stable, noble\n4) becasue it has an electrical charge since the protons (positive) and electrons (negative) are unequal.
549584
2 ATP molecules. You dont want to use to many atp molecules to make energy or the process would be too inefficient.
390298
active site interactions and the microenviroment surrounding it are more favorable to that substrate....it has a higher affinity for it.
481753
For it to be stable, the attraction of the proton has to equal the repulsion of the electrons (the neutrons have no charge). So the electrons have a negative charge, and the protons must counter with an equal positive charge to hold onto those electrons and keep it stable.
495952
Energy level is much more significant to atomic size.
267962
Lowest potential well determines the localization of the proton. Putting energy into the system, e.g., by light absorption in photosynthetic proteins, will shift the potential wells with respect to each other and proton transfer ensues. If the last member of the chain has the lowest potential, the proton gets trapped in this well. Efficient proton trans-location is deducible from the occurrence of broad negative bands in the IR difference spectrum because the proton with its large polarizability is lost.
469059
in order of increasing stability: 1, 2, 3.\n\nThe hyperconjugative and inductive effects are complimentary to each other and can not be mutually excluded.  \n\nThe empty P orbital on the carbocation interacts with the neighboring C-H sigma bonds resulting in transfer of electron density and formation of pi-bond character between the carbocation carbon and neighboring carbons.  This is the hyperconjugative effect.  The more neighbors you have, the more sharing can happen and the more stable the carbocation is.\n\nAttraction of electron density to the positively charged carbon results in induced dipoles between the carbocation carbon and its neighbors.  This allows for delocalization of the positive charge away from the carbocation carbon to its neighbors.  The neighbors become somewhat electron deficient due to electrons density herding toward the carbocation.  The more neighbors you have the more carbons the positive charge can be delocalized to and the more stable the carbocation.\n\nThe attraction of electron density referred to in the inductive argument is the partial pi bond formation in the hyperconjugation argument.