The purpose of this lab is to analyze and to become aware of the many trends that exist within a periodic table, as well as to help us develop the skills we need to accurately graph our observations. This is done by collecting data on the elements, graphing them and then finally finding a connection we see in the pattern created on the graph to the placement of the elements on the periodic table. Sergent Welsh periodic table Graph Paper Pencil Eraser Calculator Ruler 2 Coloured Pencils The data for the Atomic Radius and the First Ionization Energy of the first 36 elements was copied from the Sergent Welsh periodic table onto an observation chart. All data was rounded and expressed in three significant digits. An appropriate scale was determined …show more content…
The Noble gases have the smallest values for the atomic radius The Alkali metals have the highest values for the atomic radius The Noble gases have the highest values for the first ionization energy The Alkali metals have the smallest values for the first ionization energy The atomic radius of the transition metals are all decreasing and are doing so in a steady manner that they could all almost be connected by a curved line The ionization energy for the transition metals however are not as consistent and form little bumps on the graph The elements Beryllium, Boron, Magnesium, Aluminum, Zinc and Gallium form little peaks and troughs for both the atomic radius and the ionization energy The elements that are found on the peaks of the AR graph are the elements Hydrogen, Lithium, Sodium and Potassium. These elements are better known as the Alkali metals and are found in the far left column of the periodic table, also known as group 1. The elements that are found on the troughs of the AR graph are the elements Helium, Neon, Argon and Krypton. These elements are better known as the noble gases and are found in the far right column of the periodic table, also known as group …show more content…
The elements that are found on the peaks of the IE graph are the elements Helium, Neon, Argon and Krypton. These elements are better known as the noble gases and are found in the far right column of the periodic table, also known as group 18. This group is not the same group that had the highest atomic radius, in fact, these elements are the one’s with the lowest atomic radius, and thus are found on the trough of the AR graph. The elements that are found on the troughs of the IE graph are the elements Hydrogen, Lithium, Sodium and Potassium. These elements are better known as the Alkali metals and are found in the far left column of the periodic table, also known as group 1. This is probably because as more and more orbital shells are added to the atom, the valence electrons get further and further apart from the nucleus making it easier to remove a valence electron, thus, a low ionization energy is required. In addition, group 1 elements also have the largest atomic size in their periods, which once again means that the valence electrons are the furthest away from the nucleus, hence a low ionization energy is
4.) I noticed that there is a relationship between the ionic radius and the atomic number of the representative elements in Group 1A. The higher the atomic number, the bigger the ionic radius is. So, while hydrogen has an atomic number of 1 and Francium has an atomic number of 87, it is safe to assume that FR has a higher ionic radius. This is true; the ionic radius for Hydrogen is 0.012, and for Francium, it is 0.194.
According to the Bohr model of hydrogen atom, the kinetic and potential energies of the electrons vary as .......... .. and... distance of electron from the nucleus. respectively. where r is the The square of the wavefunction, y}, gives us the Absorption of a given amount of energy gives rise to a larger increase in entropy the the initial temperature. Orbital energies in multi-electron atoms are mere difficult to calculate due to the additional Select the correct answers from the following multiple choice questions.
Ionizing energy also increases as the elements go across the periods and also decreases when the elements go down the groups. The atomic radius does the opposite of electronegativity and ionization; it decreases as the elements go across the periods and increases when the elements go down the groups. The electronegativity increases as you go across the periods because the elements nucleus gains 1 more proton which means more protons more power to attract the electrons, the electronegativity decreases as you go down the groups because an extra shell is added every time this then causes an increase in nuclear charge due to more protons being added. This means that the nucleus is less able to attract electrons. Ionizing energy increases across a period because as the atoms radii is getting smaller the electrons get closer to the nucleus which creates a greater attraction for the electrons making it harder to remove them.
One must look to see which element has both violet and orange spectra lines. It is shown that the element Cesium is the only element that has both violet and orange spectra lines. 2. Describe two different approaches to exciting the electrons that exist in elements. Offer a specific reason why scientists use different approaches to excite the electrons of different elements.
Where as, electrons are negatively charged(Doc.3).The neutron is the dense middle of the atom(Doc.3). The protons and neutrons in the atom are in the nucleus(Doc.3). However, the electrons preside in electron clouds outside the nucleus(Doc.3). To sum up, an atom is a small structure that defines what an element is and
When excited neon enters a plasma state and glows red. Neon is the tenth element of the periodic table and the second of the noble gases. The element is not reactive because of its electron composition. Where can you find neon?
1 The hydrogen atom has one electron which can occur in 3s, 3p and 3d and since it is one electron it experiences the same nuclear charge (full nuclear charge). The effective nuclear charge felt by more than one electron in an orbital is not the same. This is due to electrons have the same charges, thus repel each other and shield the nucleus. Helium has two electrons; hence electrons repel each other and shield the nucleus. Additionally, the 1s orbital is close to the nucleus as compared to 3s orbital.
Rare earth metals are a group of 17 that are found together on the periodic table. The whole rare earth metals are made only of metals. the group consists of yttrium and the 15 lanthanide elements. The first element in row 6 is lanthanum which is where the lanthanide group got its name. The word "rare” can make you think that the world is lacking these elements but the elements are in fact relatively abundant in the Earth's crust but in limited, insufficient amounts.
Atomic radius is the distance between the nucleus and the furthest valence electron shell. The atomic radius trend decreases going across a period because of an increasing force of attraction between protons and electrons because of an increase in the number of protons. The trend increases going down a group because it gains more orbitals meaning the greater amount of shells are added (the number of shells increases). First ionization energy is the amount of energy required to remove an electron from an atom. The first ionization energy trend increases going across a period because the protons increase and require more energy to remove an electron to pull it away from the nucleus.
As atoms go down a family, they become more metallic. Since they are becoming more metallic, the atoms want to lose electrons and therefore don’t hold the electrons as tightly, also making the atom larger. Typically as elements go across a series, they decrease in
The atomic radius cannot be measured directly because the electron cloud does not have a definite boundary. So, one way to measure the size of an atom is by calculating the bond radius, which is half the distance between the nuclei of two bonded atoms. Electron shielding (down a group, not across a period), effective nuclear charge, and the energy level that the outermost electrons occupy plays an major role in determining the atomic radius. On the periodic table, the atomic radius increases down a group because the energy level of the atom down the group increases from top to bottom causing the electrons to have more energy. The effective nuclear charge remain constant down a group because of electron shielding prevents the valence electrons
Chemical Symbol Hg CAS Number 7439-97-6 Atomic Number 80 Relative Atomic Mass 200.59 Density 13.6 g.cm-3 at 20°C Melting point -38.87 °C Boiling point 356.73°C Electronic shell [ Xe ] 4f14 5d10 6s2 Lattice Structure Rhombohedral Electronegativity 2.0 on the Pauling scale CHEMISTRY OF MERCURY Relatively to other metals,
Periodic Table Summary Jordan King - Periodic Table of Harry Potter Characters The periodic table project has been one of my favorite projects so far in my school career, mostly because I was free to choose a topic that interests me. The topic I picked was Harry Potter Characters. I chose it because my all-time favorite series of books is the Harry Potter collection and it would be really handy for reference, especially for people who haven’t seen the movies or read the books. You’re welcome non-Harry Potter fans!
Selenium - The Element In 1817, Jöns Jacob Berzelius found out an unknown substance with properties similar to that of tellurium and named it as Selenium, from the Greek word Selene, which denotes goddess of the moon1. Selenium is one of the rarest elements that are found naturally in the earth’s crust. It occupies group 16 (chalcogens) of the periodic table of elements with atomic number 34 and symbol Se. Selenium exists in multiple allotropic forms but only three are recognised. The most stable form is a metallic gray crystalline hexagonal selenium, second is crystalline monoclinic selenium which is deep red in colour and the third one is amorphous selenium, which appear red in powder form and black in vitreous form.
Arsenic is present primarily as arsenate [As(V)] and arsenite [As(III)]. In both