E.which ie

Two years later, I was having trouble understanding this property after reading several pages elsewhere. Then I stumbled across this old post and got it. So to Reigel, maybe reconsider before telling someone to Google something.

Maybe they already did. That is not SO's purpose. Aerovistae, on that time, searching google would give you something like quirksmode. Tim Down's answer is so much superior than the accepted answer at the moment. JuanMendes - Googling "javascript event.

Is that something you feel is "undesireable"? Add a comment. Active Oldest Votes. Be aware that the code below should not be used for non-printable keys such as arrow keys, which you should instead detect in the keydown event: document. Improve this answer. Tim Down Tim Down k 69 69 gold badges silver badges bronze badges.

Toskan: The accepted answer was posted a few hours before mine, and may have been accepted before I posted mine. OP let Tim down by not accepting this as answer! Deprecation notice as of September KeyboardEvent. Sablefoste 3, 3 3 gold badges 35 35 silver badges 52 52 bronze badges. It does not really require Firebug, only some sort of console.

Just another note of help for all who find this will post on other e. I made a post at jQuery forums that list a good majority of e. Please look for the alternatives, such as KeyboardEvent. See more here. You should use KeyboardEvent. Anastasis Anastasis 1 1 gold badge 6 6 silver badges 23 23 bronze badges. Note that IE11 and Edge18 don't consistently implement the spec.

During an event, e : e. Click here to see a solution to Practice Problem 3 The magnitude of the first ionization energy of hydrogen can be brought into perspective by comparing it with the energy given off in a chemical reaction. When we burn natural gas, about kJ of energy is released per mole of methane consumed. The thermite reaction, which is used to weld iron rails, gives off about kJ of energy per mole of iron oxide consumed. The first ionization energy of hydrogen is half again as large as the energy given off in either of these reactions.

The first ionization energy for helium is slightly less than twice the ionization energy for hydrogen because each electron in helium feels the attractive force of two protons, instead of one. It takes far less energy, however, to remove an electron from a lithium atom, which has three protons in its nucleus.

This can be explained by noting that the outermost, or highest energy, electron on a lithium atom is in the 2 s orbital. Because the electron in a 2 s orbital is already at a higher energy than the electrons in a 1 s orbital, it takes less energy to remove this electron from the atom.

Two trends are apparent from these data. In general, the first ionization energy increases as we go from left to right across a row of the periodic table. The first ionization energy decreases as we go down a column of the periodic table. The first trend isn't surprising.

We might expect the first ionization energy to become larger as we go across a row of the periodic table because the force of attraction between the nucleus and an electron becomes larger as the number of protons in the nucleus of the atom becomes larger. The second trend results from the fact that the principal quantum number of the orbital holding the outermost electron becomes larger as we go down a column of the periodic table.

Although the number of protons in the nucleus also becomes larger, the electrons in smaller shells and subshells tend to screen the outermost electron from some of the force of attraction of the nucleus.

Furthermore, the electron being removed when the first ionization energy is measured spends less of its time near the nucleus of the atom, and it therefore takes less energy to remove this electron from the atom. The figure below shows the first ionization energies for elements in the second row of the periodic table.

Although there is a general trend toward an increase in the first ionization energy as we go from left to right across this row, there are two minor inversions in this pattern.

The first ionization energy of boron is smaller than beryllium, and the first ionization energy of oxygen is smaller than nitrogen. These observations can be explained by looking at the electron configurations of these elements. The electron removed when a beryllium atom is ionized comes from the 2 s orbital, but a 2 p electron is removed when boron is ionized. But there is an important difference in the way electrons are distributed in these atoms.

Hund's rules predict that the three electrons in the 2 p orbitals of a nitrogen atom all have the same spin, but electrons are paired in one of the 2 p orbitals on an oxygen atom. Hund's rules can be understood by assuming that electrons try to stay as far apart as possible to minimize the force of repulsion between these particles. The three electrons in the 2 p orbitals on nitrogen therefore enter different orbitals with their spins aligned in the same direction.

In oxygen, two electrons must occupy one of the 2 p orbitals. GillesC GillesC Updated so you can see it. In some IE it doesn't exists but you can assign it and use the rest of the code as expected. Sign up or log in Sign up using Google. Sign up using Facebook. Sign up using Email and Password. Post as a guest Name. Email Required, but never shown. The Overflow Blog. Does ES6 make JavaScript frameworks obsolete?

Podcast Do polyglots have an edge when it comes to mastering programming Featured on Meta. Now live: A fully responsive profile. Linked