Electron Configurations and the Periodic Table
... •The electron configuration of an atom’s highest occupied energy level generally governs the atom’s chemical properties (the highest occupied level of the noble gases contain stable octets – outer s and p orbitals are completely filled with 8 electrons. •The exception is helium (2 electrons in highe ...
... •The electron configuration of an atom’s highest occupied energy level generally governs the atom’s chemical properties (the highest occupied level of the noble gases contain stable octets – outer s and p orbitals are completely filled with 8 electrons. •The exception is helium (2 electrons in highe ...
Periodic Table Development
... Bromine is a liquid at room temperature Located on far right side of the Periodic Table C, N, O ,P, S, F, Cl, Br, I. He, Ne, Ar, Kr, Xe Semimetals or Metalloids Have properties of both metals and nonmetals Boron, Silicon, Germanium, Arsenic, Antimony Why do elements in a group have similar propertie ...
... Bromine is a liquid at room temperature Located on far right side of the Periodic Table C, N, O ,P, S, F, Cl, Br, I. He, Ne, Ar, Kr, Xe Semimetals or Metalloids Have properties of both metals and nonmetals Boron, Silicon, Germanium, Arsenic, Antimony Why do elements in a group have similar propertie ...
Unit 3 Periodic Table Vocabulary
... Alkali Metals - Any of a group of soft, white, low-density, low-melting, highly reactive metallic elements, including lithium, sodium, potassium, rubidium, cesium, and francium. Sentence: You can find alkali metals in the periodic table. ...
... Alkali Metals - Any of a group of soft, white, low-density, low-melting, highly reactive metallic elements, including lithium, sodium, potassium, rubidium, cesium, and francium. Sentence: You can find alkali metals in the periodic table. ...
Periodic Table Properties
... • There are more energy levels so distance between positive nucleus and negative electrons increases decreasing forces of attraction • Inner electrons shield the outer electrons from the full positive charge of the nucleus • Large increase from Group 18 to 1 (e.g. Ne to Na) because the single electr ...
... • There are more energy levels so distance between positive nucleus and negative electrons increases decreasing forces of attraction • Inner electrons shield the outer electrons from the full positive charge of the nucleus • Large increase from Group 18 to 1 (e.g. Ne to Na) because the single electr ...
The placement of an element on the periodic table gives clues about
... All of the elements in group 2 of the periodic table are alkaline earth metals. They are hard metallic solids and have higher melting points than alkali metals. They all have two electrons in their outer shell. Though they are also highly reactive, they are less reactive than alkali metals. They can ...
... All of the elements in group 2 of the periodic table are alkaline earth metals. They are hard metallic solids and have higher melting points than alkali metals. They all have two electrons in their outer shell. Though they are also highly reactive, they are less reactive than alkali metals. They can ...
The Periodic Table
... • Low chemical reactivity – very stable. They have no desire to gain or lose electrons! ▫ Example – He used for blimps. ▫ Typically inert – thought to be completely unreactive. Exception: 1962, chemists were able to make some compounds with Xe. ...
... • Low chemical reactivity – very stable. They have no desire to gain or lose electrons! ▫ Example – He used for blimps. ▫ Typically inert – thought to be completely unreactive. Exception: 1962, chemists were able to make some compounds with Xe. ...
the periodic law
... 7. Period trends – ionization energies of main group elements increase across each period a. Slight increase between IIA and IIIA due to p-sublevels having a higher energy so electrons are easier to remove b. Slight decrease between VA and VIA due to paired electrons in the p-sublevel. Paired e- ha ...
... 7. Period trends – ionization energies of main group elements increase across each period a. Slight increase between IIA and IIIA due to p-sublevels having a higher energy so electrons are easier to remove b. Slight decrease between VA and VIA due to paired electrons in the p-sublevel. Paired e- ha ...
The Periodic Table
... • Low chemical reactivity – very stable. They have no desire to gain or lose electrons! ▫ Example – He used for blimps. ▫ Typically inert – thought to be completely unreactive. Exception: 1962, chemists were able to make some compounds with Xe. ...
... • Low chemical reactivity – very stable. They have no desire to gain or lose electrons! ▫ Example – He used for blimps. ▫ Typically inert – thought to be completely unreactive. Exception: 1962, chemists were able to make some compounds with Xe. ...
Alkaline Earth Metals
... – Fluorine is the most reactive element in existence – This high reactivity is due to their atoms being one electron short of a full outer shell of electrons. They form -1 anions. ...
... – Fluorine is the most reactive element in existence – This high reactivity is due to their atoms being one electron short of a full outer shell of electrons. They form -1 anions. ...
Periodic Table of Elements
... 19. _____________ electrons are the electrons in the outer energy levels of an atom. 20. _____________ electrons are transferred or shared when atoms bond together. 21. The three main categories of elements are: ________________, ____________, and __________________. 22. Metals are good ____________ ...
... 19. _____________ electrons are the electrons in the outer energy levels of an atom. 20. _____________ electrons are transferred or shared when atoms bond together. 21. The three main categories of elements are: ________________, ____________, and __________________. 22. Metals are good ____________ ...
Periodic Table
... Atomic radius one-half the distance of adjacent nuclei of identical atoms that are bonded together (a measure of size of atoms) refer to fig. 6.15 pg. 175 Period Trend: Atomic radius decreases L to R* **The trend to smaller atoms across a period is caused by the increasing positive charge on t ...
... Atomic radius one-half the distance of adjacent nuclei of identical atoms that are bonded together (a measure of size of atoms) refer to fig. 6.15 pg. 175 Period Trend: Atomic radius decreases L to R* **The trend to smaller atoms across a period is caused by the increasing positive charge on t ...
C Carbon Cu Copper
... electrons in their very outermost energy level (This is called the rule of octet.) Atoms bond until this level is complete. Atoms with few valence electrons lose them during bonding. Atoms with 6, 7, or 8 valence electrons gain electrons during bonding. ...
... electrons in their very outermost energy level (This is called the rule of octet.) Atoms bond until this level is complete. Atoms with few valence electrons lose them during bonding. Atoms with 6, 7, or 8 valence electrons gain electrons during bonding. ...
Unit 13
... C Many properties of the elements change in a predictable way as you move through the periodic table. These systematic variations are called periodic trends. Î The atomic radius is the distance from the center of an atom’s nucleus to its outermost electron. C Atoms get larger going down a group. (ie ...
... C Many properties of the elements change in a predictable way as you move through the periodic table. These systematic variations are called periodic trends. Î The atomic radius is the distance from the center of an atom’s nucleus to its outermost electron. C Atoms get larger going down a group. (ie ...
The Periodic Table
... Mosley and the Periodic Law • In 1911, the English scientist Henry Moseley discovered that the elements fit into patterns better when they were arranged according to atomic number, rather than atomic weight. • The Periodic Law states that the physical and chemical properties of the elements are peri ...
... Mosley and the Periodic Law • In 1911, the English scientist Henry Moseley discovered that the elements fit into patterns better when they were arranged according to atomic number, rather than atomic weight. • The Periodic Law states that the physical and chemical properties of the elements are peri ...
File
... elements. • By the year 1700, only 13 elements had been identified and isolated. • From 1765-1775, five new elements including H, N, and O had been isolated. • As soon as elements were (are) identified, scientists begin to look for similarities and ...
... elements. • By the year 1700, only 13 elements had been identified and isolated. • From 1765-1775, five new elements including H, N, and O had been isolated. • As soon as elements were (are) identified, scientists begin to look for similarities and ...
Unit #4 Periodic Table Families Notes
... elements above and below did not seem to match. He predicted the existence of unknown elements on the basis of these blank spaces. When the unknown elements were discovered, it was found that Mendeleev had closely predicted the properties of these elements as well as where they would be discovered. ...
... elements above and below did not seem to match. He predicted the existence of unknown elements on the basis of these blank spaces. When the unknown elements were discovered, it was found that Mendeleev had closely predicted the properties of these elements as well as where they would be discovered. ...
Matter: Building Blocks of the Universe Chapter 5 Classification of
... the same number of valence electrons Family 1—Alkali—soft, silver, white, shiny—react or combine with other elements easily—never found alone in nature Family 2—Alkaline—Earth metals—very reactive Between Family 2 and 13 are the transition metals—these are the metals you are most familiar with ...
... the same number of valence electrons Family 1—Alkali—soft, silver, white, shiny—react or combine with other elements easily—never found alone in nature Family 2—Alkaline—Earth metals—very reactive Between Family 2 and 13 are the transition metals—these are the metals you are most familiar with ...
The Periodic Table - Brookwood High School
... Widely accepted because it was able to predict the existence and properties of undiscovered elements Problem: elements were being placed in groups of elements with differing properties ...
... Widely accepted because it was able to predict the existence and properties of undiscovered elements Problem: elements were being placed in groups of elements with differing properties ...
Prentice Hall Physical Science Chapter 5: The Periodic Table
... sodium chloride is an example compound when they react with metals they form salts NaF is in toothpaste CaCl2 is used to melt snow and ice AgBr is used in photographic film Group 18 (8A) - Noble Gases (p.145) unreactive called inert all but He have 8 valence electrons, He has 2 found in small amount ...
... sodium chloride is an example compound when they react with metals they form salts NaF is in toothpaste CaCl2 is used to melt snow and ice AgBr is used in photographic film Group 18 (8A) - Noble Gases (p.145) unreactive called inert all but He have 8 valence electrons, He has 2 found in small amount ...
Periodicity - Walton High
... Atomic Radius • Atomic radius generally increases as you move down a group. • The outermost orbital size increases down a group, making the atom larger. ...
... Atomic Radius • Atomic radius generally increases as you move down a group. • The outermost orbital size increases down a group, making the atom larger. ...
Periodicity - Walton High
... Atomic Radius • Atomic radius generally increases as you move down a group. • The outermost orbital size increases down a group, making the atom larger. ...
... Atomic Radius • Atomic radius generally increases as you move down a group. • The outermost orbital size increases down a group, making the atom larger. ...
Chemistry 1 Notes #10 Chapter 6 Modern Periodic Table
... electron affinity. • Electron affinity generally increases across periods. • Increasing nuclear charge along the same sublevel attracts electrons more strongly • Electron affinity generally decreases down groups. • The larger an atom’s electron cloud is, the farther away its outer electrons are from ...
... electron affinity. • Electron affinity generally increases across periods. • Increasing nuclear charge along the same sublevel attracts electrons more strongly • Electron affinity generally decreases down groups. • The larger an atom’s electron cloud is, the farther away its outer electrons are from ...
Periodicity
... • is divided into metals (left side), nonmetals (right side), and metalliods. • is arranged in rows (across) in order of increasing energy levels of valence electrons (called periods). The period number represents the energy level for that row. • is arranged in columns (down) in order of similar orb ...
... • is divided into metals (left side), nonmetals (right side), and metalliods. • is arranged in rows (across) in order of increasing energy levels of valence electrons (called periods). The period number represents the energy level for that row. • is arranged in columns (down) in order of similar orb ...
20161025131513
... 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 elementso was he the first to make a periodic tableo what does the placement of the elements reveal links betweeno how were his predictionsSection 2 V ...
... 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 elementso was he the first to make a periodic tableo what does the placement of the elements reveal links betweeno how were his predictionsSection 2 V ...
Lesson 1 - Scientist in Residence
... This lab introduces the periodic table, the structure of the atom, and how the positions of the elements in the periodic table relate to conduction and insulation. An element is a piece of matter in its simplest form. All matter (solid, liquid, gas) is made of atoms. Atoms join together to make mole ...
... This lab introduces the periodic table, the structure of the atom, and how the positions of the elements in the periodic table relate to conduction and insulation. An element is a piece of matter in its simplest form. All matter (solid, liquid, gas) is made of atoms. Atoms join together to make mole ...
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.