\chapter[Basics in Mass Spectrometry]{Basics in\\ Mass Spectrometry} \label{chap:basics-mass-spectrometry} Mass spectrometry has become a ``buzz word'' in the field of structural biology. While it has been used for long to measure the molecular mass of little molecules, its recent developments have brought it to the center of the analytical arsenal in the field of structural biology (also of ``general'' polymer science). It is now current procedure to use mass spectrometry to measure the mass of polypeptides, oligonucleotides (even complete transfer RNAs!) and saccharides, amongst other complex biomolecules. A mass spectrometer is usually described by giving to its three main different ``regions'' a name suggestive of their function: \begin{itemize} \item the source, where production of ionized analytes takes place, \item the analyzer, where the ions are electrically/magnetically ``tortured'', \item the detector, where the ions arrive, are detected and counted. \end{itemize} Before letting Mass Spectrometry in, I would like to state once for all: \emph{mass spectrometry is aware of ionized molecular species only}\dots\\ Now, \emph{enter} Mass Spectrometry\\ \renewcommand{\sectitle}{Ion Production: The Source} \section*{\sectitle} \addcontentsline{toc}{section}{\numberline{}\sectitle} Indeed, mass spectrometry cannot do anything as long as the molecule to analyze (\emph{analyte}) is not in a charged state. The process of creating an ion from an un-charged analyte is called \emph{ionization}. Well, most of the times the ionization is favored by adapting the sample's pH to a value higher/lower than the isoelectric pH of the analyte, which will elicit the appearance of (a) charge(s) onto it. In cases where the analyte cannot be charged by simple pH variations (small molecule that does not bear any ionizable chemical group), the ionization step might require --on the massist's part-- use of starker ionization techniques, like electronic impact ionization or chemical ionization. In biopolymer mass spectrometry, the pH strategy is usually considered the right way to proceed. The ionization process might involve complex charge transfer mechanisms (not fully understood yet, at least for certain ionization/desorption methods) which tend to ionize the analyte in a way not predictable by looking at the analyte's chemical structure. Ion production should not be uncoupled from one important feature of mass spectrometry: solvent evaporation --in case of liquid sample delivery to the mass spectrometer-- and sample \emph{desorption} --in case of solid state sample introduction. The general idea is that mass spectrometry works on gas phase ions. This is because it is of crucial importance, for a correct mass measurement to take place, that the analyte be \emph{totally} freed of its chemical immediate environment. That is, it should be ``naked'' in the gas phase. Equally important is the fact that ions must be capable of travelling long distances without ever encountering any other molecule in their way. This is achieved by pumping very hard in the two regions called ``analyzer'' and ``detector''. In this respect, the source is a special region because, depending on the design of the mass spectrometer, it might be partially at the atmospheric pressure during mass spectrometer operation. It is not the aim of this manual to provide insights into mass spectrometer design topics (I just would not be able to enter into the physics details!), but the general principle is that mass spectrometry involves working on gas phase ions. This is why a mass spectrometer is usually built on extremely reliable pumping technology aimed at maintaining for long periods of time (with no sudden interruption, otherwise the detector might suffer seriously) a good vacuum in the conduit in which ions must flow during operation. \renewcommand{\sectitle}{The Analyzer} \section*{\sectitle} \addcontentsline{toc}{section}{\numberline{}\sectitle} Once an ion has been generated in the gas phase, its mass should be measured. This is a complex physical process. Depending on the mass spectrometer design, the mass measurement is based on more or less complex physical events. Magnetic mass spectrometers are usually thought of as pretty complex devices; this is also the case for the Fourier transform ion cyclotronic resonance devices. An analyzer like the \emph{time of flight} analyzer is much more simple. I will refrain from trying to explain the physics of the mass measurement, just limit myself saying that --at some stage of the mass measurement process-- forces are exerted on the ions by electric/magnetic fields (incidentally, this explains why it is so important that an analyte be ionized, otherwise it would not be subject to these fields). The ionized analytes submitted to these forces have their trajectory modified in such a way that the detector should be able to quantify this modification. Roughly, this is the measurement process. \renewcommand{\sectitle}{What Is Really Measured?} \section*{\sectitle} \addcontentsline{toc}{section}{\numberline{}\sectitle} Prior to entering into some detail, it seems necessary to make a few definitions\footnote{Interesting posting signed by Ken I. Mitchelhill in the \corpname{ABRF} mailing list at \url{http://www.abrf.org/archives}, and a document published by the California Institute of Technology.}: \begin{itemize} \item unified mass scale (u): IUPAC \& IUPAP (1959-1960) agreed upon scale with 1 u equal to 1/12 the mass of the most abundant form of carbon; the dalton is taken as identical to u (but not accepted as standard nomenclature by IUPAC or IUPAP), it is abbreviaed in Da. \item a former unit was ``a.m.u.'' (\textit{i.e.} ``atomic mass unit''). It should be considered obsolete, since based on an old 1/16 of $\mathrm{^{16}O}$ standard; \item the mass of a molecule (also ``molecular mass'') is expressed in daltons. The symbol commonly used is ``M'' (not ``m''), as in ``M+H'' or ``M+Na''\dots\ Symbol ``m'' is already employed for ion mass (as in ``m/z''); \item the mass-to-charge ratio (``m/z'') of an ion is the ion's mass (in daltons) divided by the number (z) of elementary charges. Hence ``m/z'' is ``mass per charge'' and units of ``m/z'' are ``daltons per charge''; \item nominal mass: the integral sum of the nucleons in an atom (it is also the atomic mass number); \item exact (also known as accurate) mass: the sum of the masses of the protons and neutrons plus the nuclear binding energy; \end{itemize} In the previous sections I used to say that a mass spectrometer's task is to measure masses. Well, this is not 100~\% exact. A mass spectrometer actually allows to measure something else: it measures the \emph{$m$ to $z$ ratio} of the analyte, which is denoted \emph{$m/z$}. What is this ``\emph{$m$ to $z$ ratio}'' all about? Well, we said above that a mass spectrometer has to exert forces on the ions in order to determine their $m/z$. Now, let us say that we have an electric field of constant value, $E$. We also have two ions of identical masses, one bearing one charge ($q$) and the other one bearing two charges (2$q$) --positive or negative, no matter in this discussion. These two ions, when put in the same electric field $E$, will ``feel'' two different forces exerted on them: $F_1$ and $F_2$. It is possible to calculate these forces ($F_1=qE$ and $F_2=2qE$). Evidently, the ion that bears two charges is submitted to a force that is twice as intense as the one exerted on the singly charged ion. What does this mean? It means simply that the numeric result provided by the mass spectrometer is not going to be the same for both ions, since the physics of the mass spectrometer takes into account the charge level on each different analyte. Our two ions weigh exactly the same, but the mass spectrometer simply can not know that; all it knows is how a given ion reacts to the electric field it is put in. And our two ions, evidently, will react differently. When we say that a mass spectrometer measures a $m/z$ ratio, the $z$ of this ratio represents the sum of all the charges (this is a net charge!) that sit onto the analyte. But what does the $m$ stand for? The molecular mass? No! The $m$ stands for the mass of the whole analyte ion, which is --in a word-- the \emph{measured mass}. This is not the molecular mass (which would be $M$), it is the molecular mass \emph{plus/less} the mass of the chemical entity that brings the charge to the analyte. When ionizing a molecule, what happens is that something brings (or removes) a charge. In biopolymer chemistry, for example, often the ionization is a simple protonation/deprotonation. If it is a protonation, that means that an electronic doublet (on some basic group of the analyte) captures a proton. This brings the mass of a proton to the biopolymer ($\simeq$ 1 Da). Conversely, if it is a deprotonation (loss of a proton by some acidic group, say a carboxylic that becomes a carboxylate) the polymer looses the mass of a proton. Of course, if the ionization involves a single electron transfer the mass difference is going to be so feeble as to be un-measurable on a variety of mass spectrometers. Let us try to formalize this in a less verbose manner by using a sweet amino acid as an example: \begin{itemize} \item the un-ionized analyte (Glycine) has the following formula: $\mathrm{C_2H_5O_2N_1}$; \\ the molecular mass is thus $M = 75.033$ Da; \item the analyte gets protonated in the mass spectrometer: \[\mathrm{C_2H_5O_2N_1 + H \rightharpoonup\ C_2H_6O_2N_1}\] the measured mass of the ion is thus $m = 75.033 + 1.00782$ Da and the charge beared by the ion is thus $z = +1$. \item the peak value read on the mass spectrum for this analyte will thus be:\\ \[\mathrm{value} = \frac{m}{z} = \frac{M + 1.00782}{z} = 76.04\] with $z = +1$ \end{itemize} We see here that the label on the mass spectrum does not correspond to the nominal molecular mass of the analyte: the ionizing proton is ``weighed'' with the Glycine molecule. Imagine now that, by some magic, this same Glycine molecule just gets protonated a second time. Let's do exactly the same type of calculation as above, and try to predict what value will be printed onto the mass spectrum: \begin{itemize} \item the un-ionized analyte (Glycine) has the following formula: $\mathrm{C_2H_5O_2N_1}$; \\ the molecular mass is thus $M = 75.033$ Da; \item the analyte gets protonated in the mass spectrometer \emph{two times}: \[\mathrm{C_2H_5O_2N_1 + 2H \rightharpoonup\ C_2H_7O_2N_1}\] the molecular mass of the ion is thus $M = 75.033 + 2.01564$ Da and the charge beared by the ion is thus $z = +2$. \item the peak value read on the mass spectrum for this analyte will thus be:\\ \[\mathrm{value} = \frac{m}{z} = \frac{M + 2.01564}{z} = 38.52\] with $z = +2$ \end{itemize} Oh! yes!, this time it is absolutely clear that a $m/z$ is not a molecular mass! By the way, if the Glycine happened to be ionized \emph{negatively} the calculation would have been analogous to the one above, but instead of \emph{adding} the mass of the proton(s) we would have \emph{removed} it. It is that simple. Summing up all this in a few words: an ionization involves one or more charge transfer(s) and in most cases (at least in biopolymer mass spectrometry) also involves matter transfer(s). It is crucial \emph{not} to forget the matter transfer(s) when ionizing an analyte. This means that when an ionization process is described, its description ought to be complete, clearly stating three different pieces of information: \begin{itemize} \item the charge transfer (net charge that is beared by the analyte after the ionization has completed); \item the matter transfer (optional; usually something like ``+H1''); \item the ionization level (0 means ``no ionization''; usually this would be 1 for a single ionization, but might be as large as 30 if, for example, you were ionizing myoglobin with electrospray ionization (protonation). In this case the $m/z$ value would be computed this way: \[\mathrm{value} = \frac{m}{z} = \frac{M + 30\cdot\ 1.00782}{30} = \frac{16959 + 30.2346}{30} = 566.30\] with $z = +30$ \end{itemize} By now, the reader should have grasped the importance of understanding well the ionization formalisms for accurately predicting/analyzing mass spectrometric data! In the next chapters of this manual we will describe how \pxm\ works and how the user might take advantage of its powerful capabilities. In a first chapter I will introduce some general concepts around the way the program behaves. Next, in the remaining part of this manual, a chapter will be dedicated to each important \pxm\ function or characteristic. \cleardoublepage %%% Local Variables: %%% mode: latex %%% TeX-master: "polyxmass" %%% End: