Periodic Trends The Periodic table is all the elements in order by atomic number and in columns of elements with similar properties. The organization of the periodic table helps scientist by making it easy to know the properties of an element and to know how reactive the element is. The periodic table has trends that tell the scientists about the elements. Two of the trends are ionization and electron affinity. Ionization and electron affinity tell the scientist how reactive an element is. Ionization is the amount of energy it takes to take a valence electron from an element. Every element wants a full shell of valence electrons and will bond with other atoms to get it. Sodium has a lower ionization level than sulfur, because sodium has one valence electron and it would be easier to give that one away than to gain seven electrons, but sulfur has six valence electrons and it would be easier for it to gain two electrons than to lose. The more valence electrons an atom has the less it wants to give away its electrons, and the atom will have a tighter hold on the electrons which means more energy to take a valence electron. Sodium has a higher Ionization than …show more content…
Elements with more valence electrons want to gain electrons to complete their shell of valence electrons, so they have a stronger electron affinity. Sulfur wants to gain more electrons more than sodium, so the electron affinity is higher. The more rings an atom has the weaker the electron affinity is, because the valence electrons are farther away from the nucleus. Sodium has three electron rings and potassium has four electron rings, so the valence electron on sodium is closer to the nucleus and has a stronger pull to the nucleus than potassium. A valence electron from a different atom would feel the stronger pull of sodium and more likely bond with sodium than potassium. Which means that sodium has a greater electron affinity than
The chemical elements are divided into two broad groups, the metals and the non-metals. In this experiment, you will examine some members of the metal group and identify similarities and differences in their physical and chemical properties. Metals are the elements that are found in the left of the periodic table with high electrical and thermal conductivity. Metals lose electrons to create positive ion charges. Metals have a unique shine, are prone to forming, have a high tendency to form cations, and combine with oxygen to give mostly basic oxides.
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.
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.
A nucleus of an atom is accompanied by several electron shells that orbits around it. Each shell is only allowed a certain number of electrons. The first layer can hold 2, the second layer can hold 8, and the third layer can hold 18 electrons. All atoms prefer a full outer shell, however only noble gases hold them. This causes atoms to either give up or gain electrons from other atoms they encounter to have a full outer shell.
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
For example, it was found that the alkaline earth metals react with O₂ to form XO. From this information, all elements with this reaction could be classified under the second group of elements. Next density was the last deciding factor to determine which elements go into which group. This only needed to be done for hydrogen and fluorine as they were the two elements that did not follow the periodic trend of reacting with similar compounds to form similar reactants. For hydrogen, it is known it is the lightest element from looking at the periodic table, determining it to be the least dense.
Covalent bonding occurs when atoms share pairs of electrons. Another type of bonding is called a metallic bond. A metal bond is different form covalent and ionic bonds,
Fluorine has higher ionization energy than boron because fluorine’s valence electrons experience greater attraction to the nucleus. Both boron and fluorine share the same highest principal quantum number, but since fluorine has an effective nuclear charge of 2.2 and boron has an effective nuclear charge of 1.4 it will be harder to remove a valence electron from fluorine. 2c. Oxygen has lower ionization energy than nitrogen because it’s valence electrons are less attracted to the nucleus than those of nitrogen. Both nitrogen and oxygen have valence electrons at n=2, but since oxygen has a lower effective nuclear charge than that of nitrogen it will be easier to remove a valence electron, therefore requiring less energy to ionize
Halogens are group 17. Halogens are highly reactive in elemental form. Even though this group only needs one electron in its outer level, it has seven electrons. When halogens are in gas form they are diatomic molecules. Diatomic molecules are two atoms in the same covalent bonds.
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?
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
Properties of Ionic and Covalent Substances Lab Report Introduction The purpose of this lab was to determine which of the following substances: wax, sugar, and salt, are an ionic compound and which are a covalent compound. In order to accurately digest the experiments results, research of definitions of each relating led to the following information: ionic compounds are positive and negatively charged ions that experience attraction to each other and pull together in a cluster of ionic bonds; they are the strongest compound, are separated in high temperatures, and can be separated by polar water molecules. A covalent compound forms when two or more nonmetal atoms share valence electrons; covalent compounds are also
Properties of Ionic and Covalent Substances Lab Report Introduction The purpose of this lab was to determine which of the following substances: wax, sugar, and salt, are an ionic compound and which are a covalent compound. In order to accurately digest the experiments results, definitions of each relating factor were researched, leading to the following information: ionic compounds are positive and negatively charged ions that experience attraction to each other and pull together in a cluster of ionic bonds; they are the strongest compound, are separated in high temperatures, and can be separated by polar water molecules. A covalent compound is formed when two or more nonmetal atoms share valence electrons; covalent compounds are also categorized into two sections: polar covalent and nonpolar covalent. Furthermore, polar covalent compounds dissolve in water, while nonpolar covalent compounds do not.
This means there is no movement of ions in or out of the cell membrane and a resting potential is attained. At this point, there are more sodium ions outside the cell membrane and more potassium ions inside the