Periodic Table – Organizing the Elements
... –The electron to be removed from Na is further from the nucleus than Lithium’s electron. –Sodium’s electron is held more loosely and therefore easier (less energy) to remove. ...
... –The electron to be removed from Na is further from the nucleus than Lithium’s electron. –Sodium’s electron is held more loosely and therefore easier (less energy) to remove. ...
Unit 5 – The Periodic Table
... – Most reactive nonmetals • As reactive as alkali metals • Rarely free elements ...
... – Most reactive nonmetals • As reactive as alkali metals • Rarely free elements ...
The Periodic Table
... • Explain how atomic radius is measured. • Understand, identify, and discuss the trends on the periodic table for atomic radius and for electronegativity. ...
... • Explain how atomic radius is measured. • Understand, identify, and discuss the trends on the periodic table for atomic radius and for electronegativity. ...
File
... 2. Identify each element as a metal, metalloid, or nonmetal. a) fluorine b) germanium c) zinc d) phosphorous e) lithium 3. Give two examples of elements for each category. a) noble gases b) halogens c) alkali metals d) alkaline earth metals 4. The halogen family or halides form salts with which othe ...
... 2. Identify each element as a metal, metalloid, or nonmetal. a) fluorine b) germanium c) zinc d) phosphorous e) lithium 3. Give two examples of elements for each category. a) noble gases b) halogens c) alkali metals d) alkaline earth metals 4. The halogen family or halides form salts with which othe ...
Example
... Valence Numbers • Valence electrons: how many electrons are in the outer shell. • Chemically stable: elements having their outer shell full. The noble gases are chemically stable without bonding. • To fill the outer shell, elements can share or steal electrons (bond). • To be “Happy” atoms typicall ...
... Valence Numbers • Valence electrons: how many electrons are in the outer shell. • Chemically stable: elements having their outer shell full. The noble gases are chemically stable without bonding. • To fill the outer shell, elements can share or steal electrons (bond). • To be “Happy” atoms typicall ...
Chapter 6- The Periodic Table
... well an atom can attract electrons from another atom to which it is bonded. • They are already bonded...what does it do to the electrons. The more electronegative it is, the more likely it is to pull off electrons of its partner. ...
... well an atom can attract electrons from another atom to which it is bonded. • They are already bonded...what does it do to the electrons. The more electronegative it is, the more likely it is to pull off electrons of its partner. ...
The Periodic Table
... Ionization energy greatly increases when you start removing electrons from an inner shell (n decreases). Moving across a period, two other factors come into play: • “p” e– ’s are higher energy… require less energy to remove than “s” e– ’s with the same quantum number, n • e– ’s in filled orbitals ar ...
... Ionization energy greatly increases when you start removing electrons from an inner shell (n decreases). Moving across a period, two other factors come into play: • “p” e– ’s are higher energy… require less energy to remove than “s” e– ’s with the same quantum number, n • e– ’s in filled orbitals ar ...
The Periodic Table - TangHua2012-2013
... indicating missing elements (not discovered yet). Why was this important? • The location of missing elements allowed their chemical and physical properties to be predicted. ...
... indicating missing elements (not discovered yet). Why was this important? • The location of missing elements allowed their chemical and physical properties to be predicted. ...
AP Chemistry – Chapter 7 Reading Guide: Periodic Table of the
... 4. Explain the periodic trend for Zeff and how it relates to atomic radius, ionization energy, and electronegativity. (Please note how much room you have to answer this question) ...
... 4. Explain the periodic trend for Zeff and how it relates to atomic radius, ionization energy, and electronegativity. (Please note how much room you have to answer this question) ...
The Periodic Table
... grouped into families. Families may be one column, or several columns put together. Families have names rather than numbers. (Just like your family has a common last name.) ...
... grouped into families. Families may be one column, or several columns put together. Families have names rather than numbers. (Just like your family has a common last name.) ...
20151023082664
... o what patterns did he noticeo what was his final arrangement of the periodic tableo what was missing in his tableo how did he predict undiscovered elements o was he the first to make a periodic tableo what does the placement of the elements reveal links betweeno how were his predictionsSection 2 ...
... o what patterns did he noticeo what was his final arrangement of the periodic tableo what was missing in his tableo how did he predict undiscovered elements o was he the first to make a periodic tableo what does the placement of the elements reveal links betweeno how were his predictionsSection 2 ...
Ch. 11.4 Notes (Periodicity) teacher 2012
... – Also, moving across a period takes us from metals to anions nonmetals. Since nonmetals generally form _________, they gain tend to __________ e-’s anyway, and this makes them highly ________________ attracted to e-’s when forming a chemical bond. Noble __________ gases – ___________ are not listed ...
... – Also, moving across a period takes us from metals to anions nonmetals. Since nonmetals generally form _________, they gain tend to __________ e-’s anyway, and this makes them highly ________________ attracted to e-’s when forming a chemical bond. Noble __________ gases – ___________ are not listed ...
III. Periodic Trends
... 1. Electron affinity slightly decreases down a group. 2. Electron affinity generally tends to increase across a period. ...
... 1. Electron affinity slightly decreases down a group. 2. Electron affinity generally tends to increase across a period. ...
File
... 6. What properties to metals, nonmetals, and metalloids have? Metals - Shiny luster, malleable, some are magnetic, good conductors of electricity and heat. Nonmetals – dull luster, brittle, nonmagnetic, insulators. Metalloids- properties of both, sometimes called semi-conductors. ...
... 6. What properties to metals, nonmetals, and metalloids have? Metals - Shiny luster, malleable, some are magnetic, good conductors of electricity and heat. Nonmetals – dull luster, brittle, nonmagnetic, insulators. Metalloids- properties of both, sometimes called semi-conductors. ...
6-1-Periodic Law
... It was found that if Mendeleev's table was ordered by atomic number instead of atomic mass the inconsistencies in the table were eliminated. This is the blueprint for the modern periodic table. ...
... It was found that if Mendeleev's table was ordered by atomic number instead of atomic mass the inconsistencies in the table were eliminated. This is the blueprint for the modern periodic table. ...
6.6 – Periodic Table
... 6.6 – Periodic Table Physical Properties of the Periodic Table Metals – Excellent conductors of heat and electricity. Often ductile (able to be squeezed out into a wire) and malleable (able to be hammered into sheets). Tend to lose electrons (or become positively charged). Can be mixed with other m ...
... 6.6 – Periodic Table Physical Properties of the Periodic Table Metals – Excellent conductors of heat and electricity. Often ductile (able to be squeezed out into a wire) and malleable (able to be hammered into sheets). Tend to lose electrons (or become positively charged). Can be mixed with other m ...
Periodic Table Timeline
... Hennig Brand becomes the first known discoverer of an element, phosphorus, from distilled human urine. ...
... Hennig Brand becomes the first known discoverer of an element, phosphorus, from distilled human urine. ...
Chemistry 101 Topic 4
... • Gives the # of atoms and how the atoms are connected to one another. The atoms in molecules have specific arrangements because they are held together by a:rac2ve forces called bonds. A bond is ...
... • Gives the # of atoms and how the atoms are connected to one another. The atoms in molecules have specific arrangements because they are held together by a:rac2ve forces called bonds. A bond is ...
The Periodic Table
... reactive. Due to their e high reactivity (electronegativity), they are not found in their elemental form in any natural environment on Earth. They are generally toxic, or even lethal, to biological organisms in their elemental forms. ...
... reactive. Due to their e high reactivity (electronegativity), they are not found in their elemental form in any natural environment on Earth. They are generally toxic, or even lethal, to biological organisms in their elemental forms. ...
Parts of the Periodic Table
... • EX: Calcium (Ca) will react vigorously upon contact with water, but will not explode like sodium. ...
... • EX: Calcium (Ca) will react vigorously upon contact with water, but will not explode like sodium. ...
Periodic Table Trends
... Elements in Group VII have very similar properties because their atoms all have seven valence electrons. As in Group II, as one moves down Group VII the number of occupied shells increases. In this group, however, the greater the ‘shielding’ effect the less readily the atom will gain an electron in ...
... Elements in Group VII have very similar properties because their atoms all have seven valence electrons. As in Group II, as one moves down Group VII the number of occupied shells increases. In this group, however, the greater the ‘shielding’ effect the less readily the atom will gain an electron in ...
1 - DarringtonScience
... What physical and chemical properties are found among the nonmetals? What happens to the atoms of most nonmetals when they react with other elements? How do the physical and chemical properties of halogens compare with those of the noble gases? Where in the periodic table are the metalloids found? ...
... What physical and chemical properties are found among the nonmetals? What happens to the atoms of most nonmetals when they react with other elements? How do the physical and chemical properties of halogens compare with those of the noble gases? Where in the periodic table are the metalloids found? ...
Chapter 5: Atomic Structure and The Periodic Table
... protons, neutrons, and electrons in an atom. ...
... protons, neutrons, and electrons in an atom. ...
Noble gas
The noble gases make a group of chemical elements with similar properties. Under standard conditions, they are all odorless, colorless, monatomic gases with very low chemical reactivity. The six noble gases that occur naturally are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and the radioactive radon (Rn).For the first six periods of the periodic table, the noble gases are exactly the members of group 18 of the periodic table.It is possible that due to relativistic effects, the group 14 element flerovium exhibits some noble-gas-like properties, instead of the group 18 element ununoctium. Noble gases are typically highly unreactive except when under particular extreme conditions. The inertness of noble gases makes them very suitable in applications where reactions are not wanted. For example: argon is used in lightbulbs to prevent the hot tungsten filament from oxidizing; also, helium is breathed by deep-sea divers to prevent oxygen and nitrogen toxicity.The properties of the noble gases can be well explained by modern theories of atomic structure: their outer shell of valence electrons is considered to be ""full"", giving them little tendency to participate in chemical reactions, and it has been possible to prepare only a few hundred noble gas compounds. The melting and boiling points for a given noble gas are close together, differing by less than 10 °C (18 °F); that is, they are liquids over only a small temperature range.Neon, argon, krypton, and xenon are obtained from air in an air separation unit using the methods of liquefaction of gases and fractional distillation. Helium is sourced from natural gas fields which have high concentrations of helium in the natural gas, using cryogenic gas separation techniques, and radon is usually isolated from the radioactive decay of dissolved radium, thorium, or uranium compounds (since those compounds give off alpha particles). Noble gases have several important applications in industries such as lighting, welding, and space exploration. A helium-oxygen breathing gas is often used by deep-sea divers at depths of seawater over 55 m (180 ft) to keep the diver from experiencing oxygen toxemia, the lethal effect of high-pressure oxygen, and nitrogen narcosis, the distracting narcotic effect of the nitrogen in air beyond this partial-pressure threshold. After the risks caused by the flammability of hydrogen became apparent, it was replaced with helium in blimps and balloons.