u4_tqs - Teach-n-Learn-Chem
... 31. Why are the electrons drawn closer to the nucleus when a sodium atom loses an electron? the attraction between the remaining electrons and the nucleus is increased 32. As the number of electrons increases, the attraction of the ...
... 31. Why are the electrons drawn closer to the nucleus when a sodium atom loses an electron? the attraction between the remaining electrons and the nucleus is increased 32. As the number of electrons increases, the attraction of the ...
Periodic Table and Trends
... Defined by an atoms tendency to attract electrons in a chemical bond. In a chemical bond, atoms have to share electrons The atom with a higher electronegativity will keep the electrons closer to it. ...
... Defined by an atoms tendency to attract electrons in a chemical bond. In a chemical bond, atoms have to share electrons The atom with a higher electronegativity will keep the electrons closer to it. ...
Textbook Questions - Teach-n-Learn-Chem
... 30. Cations are always __________ than the atoms from which they form; anions are always _________. 31. Why are the electrons drawn closer to the nucleus when a sodium atom loses an electron? ...
... 30. Cations are always __________ than the atoms from which they form; anions are always _________. 31. Why are the electrons drawn closer to the nucleus when a sodium atom loses an electron? ...
File
... valence shell of a gaseous atom or ion in the ground state. Across a period, IE increases because electrons are more tightly bound to the nucleus (more p+ in the nucleus). Down a group, IE decreases because electrons are farther from the nucleus and not held as tight. Values are found on Table S ...
... valence shell of a gaseous atom or ion in the ground state. Across a period, IE increases because electrons are more tightly bound to the nucleus (more p+ in the nucleus). Down a group, IE decreases because electrons are farther from the nucleus and not held as tight. Values are found on Table S ...
ELEMENTS
... - In the modern periodic table, all the elements are arranged in order of ___________ atomic number. - 1.The group number of an element is equal to the number of outermost shell electrons of its atoms. ** Group number = number of ____________________ ** 2. Elements in the same vertical column (calle ...
... - In the modern periodic table, all the elements are arranged in order of ___________ atomic number. - 1.The group number of an element is equal to the number of outermost shell electrons of its atoms. ** Group number = number of ____________________ ** 2. Elements in the same vertical column (calle ...
Chapter 4
... representative elements because metals, nonmetals, metalloids, and noble gases are all represented ...
... representative elements because metals, nonmetals, metalloids, and noble gases are all represented ...
Chapter 7
... 2. Explain the relationship between valence electron configurations and the organization of the periodic table. You should be able to: • demonstrate that elements in a group have similar valence electron configurations 3. Write the electron configuration for ions up to Z = 36, including ions of repr ...
... 2. Explain the relationship between valence electron configurations and the organization of the periodic table. You should be able to: • demonstrate that elements in a group have similar valence electron configurations 3. Write the electron configuration for ions up to Z = 36, including ions of repr ...
Unit 8 Summary
... Dobereiner – 1817, organized the known elements into triads (groups of 3) based on appearance and reactions Newlands – 1864, organized the known elements into octaves (groups of 8) based on properties Mendeleev – 1869, considered the father of the modern periodic table; organized the known elements ...
... Dobereiner – 1817, organized the known elements into triads (groups of 3) based on appearance and reactions Newlands – 1864, organized the known elements into octaves (groups of 8) based on properties Mendeleev – 1869, considered the father of the modern periodic table; organized the known elements ...
Atoms, Bonding, and the Periodic Table Electron Dot Diagrams
... The valence electrons of an atom are shown as dots around the symbol of the element. Complete the electron dot diagram for neon. ...
... The valence electrons of an atom are shown as dots around the symbol of the element. Complete the electron dot diagram for neon. ...
Periodic Table Workshop
... atomic size increases, e- from higher energy levels are "shielded*" from the nucleus and are therefore not as tightly bound. (the "*shielding effect") • left to right: increases, as elem's closer to group 7 tend to want to gain e-'s. (Noble gases have the highest F.I.E.) ...
... atomic size increases, e- from higher energy levels are "shielded*" from the nucleus and are therefore not as tightly bound. (the "*shielding effect") • left to right: increases, as elem's closer to group 7 tend to want to gain e-'s. (Noble gases have the highest F.I.E.) ...
Periodic TABLE: Tables: PT, Table S
... group have the same number of valence electrons (helium is an exception) and therefore similar chemical properties. 3.1aaThe succession of elements within the same group demonstrates characteristic trends: differences in atomic radius, ionic radius, electronegativity, first ionization energy, metall ...
... group have the same number of valence electrons (helium is an exception) and therefore similar chemical properties. 3.1aaThe succession of elements within the same group demonstrates characteristic trends: differences in atomic radius, ionic radius, electronegativity, first ionization energy, metall ...
Standard EPS Shell Presentation
... gases or liquids in their pure form. Fluorine (F), chlorine (Cl), and bromine (Br) form salts when the bond with alkali metals. ...
... gases or liquids in their pure form. Fluorine (F), chlorine (Cl), and bromine (Br) form salts when the bond with alkali metals. ...
File
... [Nitrogen, Oxygen, Argon] has a full valence shell and is a noble gas. Noble gases are [inert, very reactive, only react with certain elements]. [Potassium, Calcium, Sulfur, Neon] has properties most similar to oxygen. [Calcium, Potassium, Chlorine, Sodium] has two valence electrons. Periods form [h ...
... [Nitrogen, Oxygen, Argon] has a full valence shell and is a noble gas. Noble gases are [inert, very reactive, only react with certain elements]. [Potassium, Calcium, Sulfur, Neon] has properties most similar to oxygen. [Calcium, Potassium, Chlorine, Sodium] has two valence electrons. Periods form [h ...
6-Getting to Know the Periodic Table
... Complete the following objectives using the periodic table below. ...
... Complete the following objectives using the periodic table below. ...
Periodic Table Cloze - Science
... _________________ is a form of matter that is composed of a single type of _________________. In 1869, Dmitri _________________ created the Calcium: an element on the periodic table with atomic number 20. ...
... _________________ is a form of matter that is composed of a single type of _________________. In 1869, Dmitri _________________ created the Calcium: an element on the periodic table with atomic number 20. ...
Chapter 8 Study Guide
... Most of the elements are classified as metals. Properties of elements change as you go across a period. Alkali Metals I- most reactive metals Alkaline Earth Metals II- not as reactive as Alkali Metals Halogens (VII)- most reactive non-metals; “salt formers” Noble Gases (VIII)- colorless, odorless ga ...
... Most of the elements are classified as metals. Properties of elements change as you go across a period. Alkali Metals I- most reactive metals Alkaline Earth Metals II- not as reactive as Alkali Metals Halogens (VII)- most reactive non-metals; “salt formers” Noble Gases (VIII)- colorless, odorless ga ...
Periodic Properties
... ii) Nonmetals are at the right of the Table. They tend to be insulators and react easily with metals. iii) Metalloids separate the metals and nonmetals and have intermediate properties iv) Noble Gases exist at the extreme right, are chemically stable and have full valence shells ...
... ii) Nonmetals are at the right of the Table. They tend to be insulators and react easily with metals. iii) Metalloids separate the metals and nonmetals and have intermediate properties iv) Noble Gases exist at the extreme right, are chemically stable and have full valence shells ...
File
... Elements are listed horizontally according to their atomic number - number of protons Periods are the horizontal rows of elements Halogens - highly reactive, Elements are listed vertically according to their chemical properties gases except Br liquid Groups or Families are arranged vertically Noble ...
... Elements are listed horizontally according to their atomic number - number of protons Periods are the horizontal rows of elements Halogens - highly reactive, Elements are listed vertically according to their chemical properties gases except Br liquid Groups or Families are arranged vertically Noble ...
Name - Haverford Alchemy
... Active Chemistry –Chapter #1-Fun with the Periodic Table - Activity #7 Goal #2 Relate the positions of elements on the periodic table, their electron arrangements, and their distances from the nearest noble gas, to chemical properties of the elements. 2. a) The noble gases are chemically inactive m ...
... Active Chemistry –Chapter #1-Fun with the Periodic Table - Activity #7 Goal #2 Relate the positions of elements on the periodic table, their electron arrangements, and their distances from the nearest noble gas, to chemical properties of the elements. 2. a) The noble gases are chemically inactive m ...
![Periodic Table[1]](http://s1.studyres.com/store/data/003104404_1-7138f0e5d3dcc06b9019743402d7e0ca-300x300.png)
Periodic Table[1]
... Chemical properties of each vertical group or “family” are similar due to the number of electrons in their outer energy level. ...
... Chemical properties of each vertical group or “family” are similar due to the number of electrons in their outer energy level. ...
The periodic table as we have it today has not always
... The periodic table as we have it today has not always existed; it developed much in the same way as atomic theory did. In the early 1800’s scientists began looking for ways to classify the elements that had been discovered. ...
... The periodic table as we have it today has not always existed; it developed much in the same way as atomic theory did. In the early 1800’s scientists began looking for ways to classify the elements that had been discovered. ...
Unit 10: Chemical Periodicity
... trends in atomic radii, ionization energy, electronegativity and reasons for these trends why electronegativity and ionization follow same trend recall jumps in multiple ionization energies how to determine # of electrons in outermost energy level relationship between size of ions and the ...
... trends in atomic radii, ionization energy, electronegativity and reasons for these trends why electronegativity and ionization follow same trend recall jumps in multiple ionization energies how to determine # of electrons in outermost energy level relationship between size of ions and the ...
here
... electronegativity count valence electrons how ions form bonding the octet rule the nature of the ionic bond the nature of the covalent bond single, double, and triple bonds Lewis structures octet rule draw Lewis structures from formulas exceptions to the octet rule VSEPR Theory from the chemical for ...
... electronegativity count valence electrons how ions form bonding the octet rule the nature of the ionic bond the nature of the covalent bond single, double, and triple bonds Lewis structures octet rule draw Lewis structures from formulas exceptions to the octet rule VSEPR Theory from the chemical for ...
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.