Question #3578d
Caesium is a chemical element with atomic number 55 which means there are 55 protons and 55 electrons in the atomic structure. The chemical symbol for Caesium is Cs. Caesium is a soft, silvery-gold alkali metal with a melting point of 28.5 °C, which makes it one of only five elemental metals that are liquid at or near room temperature. Caesium(1+) is a caesium ion, a monovalent inorganic cation, a monoatomic monocation and an alkali metal cation. 1 Structures Expand this section.
1 Answer
Explanation:
The question wants you to recognize the fact that cesium,
With the exception of hydrogen, elements located in group 1 of the periodic table are called alkali metals and are all characterized by the fact that they have one valence electron.
That is, these elements have one electron located in their outermost shell, i.e their valence shell. As you know, chemical reactivity is governed by an atom's 'desire' to acquire eight electrons in its outermost shell
In order to complete their octet, these elements lose that outermost electron. This means that they will only react with elements that are 'interested' in taking the electron that the alkali metals are offering.
Cesium will thus not react with another element that is interested in giving away electrons in order to complete its octet, i.e. with another metal.
As you can see from the options given to you, barium,
On the other hand, iodine,
Cesium Has How Many Valence Electrons
That happens because iodine has seven valence electrons, which means that it only needs one to complete its octet.
Therefore, when cesium reacts with iodine, it gives its valence electron to iodine, becoming positively charged in the process, i.e. a cesium cation,
Iodine will pick up this electron and become negatively charged in the process, i.e. an iodide anion,
These two ions will then be attracted to each other by the electrostatic force of attraction
Related questions
As mentioned above, the characteristic chemical property of a metalatom is to lose one or more of its electrons to form a positive ion. However, certain metals lose electrons much more readily than others. In particular, cesium (Cs) can give up its valence electron more easily than can lithium (Li). In fact, for the alkali metals (the elements in Group 1), the ease of giving up an electron varies as follows: Cs > Rb > K > Na > Li with Cs the most likely, and Li the least likely, to lose an electron. In going down the group, the metals become more likely to lose an electron because the electron being removed lies increasingly farther from the positive nucleus. That is, the electron lost from Cs to form Cs+ lies at a much greater distance from the attractive positive nucleus—and is thus easier to remove—than the electron that must be removed from a lithium atom to form Li+. The same trend also is seen among the Group 2 elements (the alkaline-earth metals); the farther down in the group the metal resides, the more likely it is to lose an electron.
Just as metals vary somewhat in their properties, so do nonmetals. As a general rule, the most chemically active metals appear in the lower left-hand region of the periodic table, whereas the most chemically active nonmetals appear in the upper right-hand region. The properties of the semimetals, or metalloids, lie between those of the metals and the nonmetals.
The ionization energy of an element is the energy required to remove an electron from an individual atom. Here M(g) represents a metal in the vapour state.
Metal atoms lose electrons to nonmetal atoms because metals typically have relatively low ionization energies. Metals at the bottom of a group lose electrons more easily than those at the top. That is, ionization energies tend to decrease in going from the top to the bottom of a group. Nonmetals, which are found in the right-hand region of the periodic table, have relatively large ionization energies and therefore tend to gain electrons. Ionization energies generally increase in going from left to right across a given period. Thus, the elements that appear in the lower left-hand region of the periodic table have the lowest ionization energies (and are therefore the most chemically active metals), while the elements that occur in the upper right-hand region of the periodic table have the highest ionization energies (and are thus the most chemically active nonmetals).
As mentioned above, when a nonmetallic element reacts with a metallic element, electrons are transferred from the atoms of the metal to the atoms of the nonmetal, forming positive ions (cations) and negative ions (anions), respectively. This produces an ionic compound. For example, lithium and fluorine (F) react to form lithium fluoride (LiF), which contains Li+ and F− ions.
In contrast, when two nonmetallic elements react, the atoms combine to form molecules by sharing electrons. Bonds formed by electron sharing between atoms are called covalent bonds. The electrons are shared rather than transferred, because the two nonmetal atoms have comparable attractive powers for the electrons in the bond. For example, fluorinegas consists of F2 molecules in which the fluorine atoms are bound together by sharing a pair of electrons, one contributed by each atom. In addition, hydrogen and fluorine react to form hydrogen fluoride, which contains HF molecules. The hydrogen and fluorine atoms are bound together by a pair of electrons, one electron contributed by the hydrogen atom and one by the fluorine atom. Although the electrons are shared between the hydrogen and the fluorine atoms, in this case they are not shared equally. This is clear from the fact that the HF molecule is polar; the hydrogen atom has a partial positive charge (δ+), while the fluorine atom has a partial negative charge (δ−): H―F
δ+ δ− (In this example the symbol δ stands for a number less than one.) This electrical polarity occurs because the shared electrons spend more time close to the fluorine atom than to the hydrogen atom. That is, fluorine has greater affinity for the shared electrons than does hydrogen. This leads to a polar covalent bond.
The ability of an atom to attract the electrons shared with another atom is termed its electronegativity. The relative electronegativities of the various atoms can be determined by measuring the polarities of the bonds involving the atoms in question. Fluorine has the greatest electronegativity value (4.0, according to the Pauling scale), and cesium and francium have the smallest values (0.79 and 0.7, respectively). In general, nonmetal atoms have higher electronegativities than metal atoms. In the periodic table, electronegativity typically increases in moving across a period and decreases in going down a group. When elements with very different electronegativities (such as fluorine and cesium) react, one or more electrons are transferred to form an ionic compound. For example, cesium and fluorine react to form CsF, which contains Cs+ and F− ions. When nonmetal atoms with differing electronegativities react, they form molecules with polar covalent bonds.
Cesium Element Valence Electrons
Another important atomic property is atomic size. The sizes of atoms vary; atoms generally tend to become larger in going down a group on the periodic table and smaller in going from left to right across a period.