The chemical reactivity of transition metals is generally less than that of metals to its left (group 1 and group 2 metals). However, transition metals can exhibit various oxidation states and hence form more number of compounds than group 1 and group 2 elements.
They are organized according to atomic number, which refers to the number of protons that the nucleus contains. They are organized into columns, called families by the number of electrons in the orbitals. The farther down you go, the more elements, because there are more orbitals on higher energy levels. Also, the elements to the right of the line on the periodic table are nonmetals, the ones on the line are semimetals, and the ones to the left of the line are metals.
The group proposing that elements within the same group have the same electron configurations in their valence shell, which is the most important factor in accounting for their similar properties. Elements in the same group also show patterns in their atomic radius, ionization energy, and electronegativity. From top to bottom in a group, the atomic radii of the elements increase. Since there are more filled energy levels, valence electrons are found farther from the nucleus. From the top, each successive element has a lower ionization energy because it is easier to remove an electron since the atoms are less tightly bound. Similarly, a group will also see a top to bottom decrease in electronegativity due to an increasing distance between valence electrons and the nucleus. While, the elements in the same period show trends in atomic radius, ionization energy, electron affinity, and electronegativity. Moving left to right across a period, atomic radius usually decreases. This occurs because each successive element has an added proton and electron which causes the electron to be drawn closer to the nucleus. This decrease in atomic radius also causes the ionization energy to increase when moving from left to right across a period. The more tightly bound an element is, the more energy is required to remove an electron. Similarly, electronegativity will increase in the same manner as ionization energy because of the amount of pull that is exerted on the electrons by the nucleus. Electron affinity also shows a slight trend across a period. Metals (left side of a period) generally have a lower electron affinity than nonmetals (right side of a period) with the exception of the noble gases.
In addition to hydrogen, all elements in Group I of the periodic table have one valence electron. They are lithium, sodium, potassium, rubidium, cesium, and francium. The farther you move right on the periodic table the more valence electrons. For example, elements in Group VII have 8 valence electrons except helium.
"higher energy"
The name of the group is the oxygen family. The valence number for elements in that group are -2. (gain or share two electrons) Oxygen, sulfur and selenium are nonmetals. Tellurium and Polonium are metalloids.
As you pass from left to right and from one line to the next line below it, you are incrreasing the atomic number of each element, one proton at a time. As the protons increase, so do the electrons, and they fill up shells and start new shells. Chemical properties depend mainly on the number of electrons in the outermost shell (for transition state elements it doesn't work exactly by shells, since in the heavier elements it is possible for an electron in an inner shell to nonetheless be farther from the nucleus than some electrons in the outer shell, but that is an added complication). So, elements in the same group have the same number of outer, or valance electrons as they are known.
The elements that are commonly recognized as metalloids or semimetals are boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), and tellurium (Te). These elements exhibit properties of both metals and nonmetals, such as being good conductors of electricity but also brittle and less malleable.
Elements from Group 3 to 12 are called Transition Elements. These elements are heavy metals. They lie between the strongly eloctropositive elements to their right and the electronegative elements ( non-metals) to their left.These metals mainly have 2 valence electronswith the metallic character decreasing from left to right of their period.
it is older
it is older
Whatever is farther to the right is greater.
they get more electrons the farther right the get
when the elements in the drawing or painting decreases. things appear smaller as they get farther
when the elements in the drawing or painting decreases. things appear smaller as they get farther
europe and rusiia are double the size of the us
The elements with low electronegativity are the metals, specifically the alkali metals and alkali earth metals. The elements further to the left of the periodic table will have lower electronegativity than those farther to the right.
The Earth moves faster than the planets that are farther from the Sun.