Electron Energy Level
... • Atoms get a positive charge when they lose electrons • Atoms get a negative charge when they gain electrons • Ionization is the process that results in the formation of an ion. ...
... • Atoms get a positive charge when they lose electrons • Atoms get a negative charge when they gain electrons • Ionization is the process that results in the formation of an ion. ...
Chapter 2:Tutorial Q: (a) What is an isotope? (b) Why are the atomic
... Ionic--there is electrostatic attraction between oppositely charged ions. Covalent--there is electron sharing between two adjacent atoms such that each atom assumes a stable electron configuration. ...
... Ionic--there is electrostatic attraction between oppositely charged ions. Covalent--there is electron sharing between two adjacent atoms such that each atom assumes a stable electron configuration. ...
Ch. 6 - The Periodic Table
... Transition Elements There are two types of transition elements—transition metals and inner transition metals. They are classified based on their electron configurations. ...
... Transition Elements There are two types of transition elements—transition metals and inner transition metals. They are classified based on their electron configurations. ...
Chapter 6
... -gases or brittle solids, dull surfaces, used as insulators -have 5 or more electrons in outer energy level ...
... -gases or brittle solids, dull surfaces, used as insulators -have 5 or more electrons in outer energy level ...
The Periodic Law Notes (Chapter 5) – Part 2
... number of valence electrons increases (the amount of energy needed to remove one electron is less then what is needed to remove 7 or 8 electrons). 3. Group trend – ionization energy increases as you move up a group (or decreases as you move down a group). In general, as you do down a group the ioniz ...
... number of valence electrons increases (the amount of energy needed to remove one electron is less then what is needed to remove 7 or 8 electrons). 3. Group trend – ionization energy increases as you move up a group (or decreases as you move down a group). In general, as you do down a group the ioniz ...
Chapter 4- The Periodic Table Section 1
... Transition metals- one of the metals that can use the inner shell before using the outer shell in a bond ...
... Transition metals- one of the metals that can use the inner shell before using the outer shell in a bond ...
Chapter 5: What you should know when you finish. Describe the
... The most reactive metals are on the left side of the table. The most reactive nonmetals are on the right in Group 17. The Period 3 elements provide an example of this trend: If you were unwise enough to hold a piece of sodium in your hand, it would react quickly and violently with the water on ...
... The most reactive metals are on the left side of the table. The most reactive nonmetals are on the right in Group 17. The Period 3 elements provide an example of this trend: If you were unwise enough to hold a piece of sodium in your hand, it would react quickly and violently with the water on ...
Chapter 6 Review Name Period _____ Know the history
... The atomic radius decreases, as you go across a period the valence electrons increase, causing a larger interaction with the nucleus 25. What is the shielding affect? The electrons that are in between the valence shell and the nucleus shield Know the trend for ionic radius. 26. What is the charge ...
... The atomic radius decreases, as you go across a period the valence electrons increase, causing a larger interaction with the nucleus 25. What is the shielding affect? The electrons that are in between the valence shell and the nucleus shield Know the trend for ionic radius. 26. What is the charge ...
1 February 04, 2016
... - old labelling system: Roman numerals followed by the letter A or B - includes elements with similar chemical properties - the elements in a group have the same number of electrons in the outermost shell/orbit - the electrons in the outermost shell are called the valence numbers ...
... - old labelling system: Roman numerals followed by the letter A or B - includes elements with similar chemical properties - the elements in a group have the same number of electrons in the outermost shell/orbit - the electrons in the outermost shell are called the valence numbers ...
Page|1 - askIITians
... Q18. Which of the following series of elements is correct in terms of increasing atomic radii? ...
... Q18. Which of the following series of elements is correct in terms of increasing atomic radii? ...
Periodic Table of Elements
... • They have 7 valence electrons and are the most reactive non-metals. • They only need to gain 1 electron and are not found as free atoms in nature. • They often combine with the transition metals. • Examples: Cl, I, and Br ...
... • They have 7 valence electrons and are the most reactive non-metals. • They only need to gain 1 electron and are not found as free atoms in nature. • They often combine with the transition metals. • Examples: Cl, I, and Br ...
Bohr Model Activity
... a. Write the symbol for the element in the centre of the atom b. Below the symbol write the number of protons (For example write 15 P) and the number of neutrons (eg. 16 N). c. Write the atomic number below the drawing. d. Highlight the outer most shell with one colour. e. Use a different colour to ...
... a. Write the symbol for the element in the centre of the atom b. Below the symbol write the number of protons (For example write 15 P) and the number of neutrons (eg. 16 N). c. Write the atomic number below the drawing. d. Highlight the outer most shell with one colour. e. Use a different colour to ...
The Periodic Law
... • More than 60 elements had been discovered. • There was no method to accurately determine an elements atomic mass or number of atoms of an element in a compound. • 1860, Germany, first international congress of chemists ...
... • More than 60 elements had been discovered. • There was no method to accurately determine an elements atomic mass or number of atoms of an element in a compound. • 1860, Germany, first international congress of chemists ...
PERIODIC TRENDS PRACTICE QUIZ
... 10. The measure of the attraction that an atom has for electrons involved in chemical bonds is known as a. Radioactivity. b. Ionization Energy. c. Electronegativity. d. Electron Affinity. ...
... 10. The measure of the attraction that an atom has for electrons involved in chemical bonds is known as a. Radioactivity. b. Ionization Energy. c. Electronegativity. d. Electron Affinity. ...
PERIODIC TRENDS PRACTICE QUIZ
... 10. The measure of the attraction that an atom has for electrons involved in chemical bonds is known as a. Radioactivity. b. Ionization Energy. c. Electronegativity. d. Electron Affinity. ...
... 10. The measure of the attraction that an atom has for electrons involved in chemical bonds is known as a. Radioactivity. b. Ionization Energy. c. Electronegativity. d. Electron Affinity. ...
II. Ch. 5.2: Electron Configuration and the Periodic Table
... Atom with highest electronegativity is ___________________. Fluorine’s value is 4. ...
... Atom with highest electronegativity is ___________________. Fluorine’s value is 4. ...
Chapter 6 PowerPoint
... Metals tend to LOSE electrons, from their outer energy level • Sodium loses one: there are now more protons (11) than electrons (10), and thus a positively charged particle is formed = “cation” • The charge is written as a number followed by a plus sign: Na1+ • Now named a “sodium ion” ...
... Metals tend to LOSE electrons, from their outer energy level • Sodium loses one: there are now more protons (11) than electrons (10), and thus a positively charged particle is formed = “cation” • The charge is written as a number followed by a plus sign: Na1+ • Now named a “sodium ion” ...
Periodic Table Notes Fill In
... 14. Where are the Transition Metals located? ______________________________________ 15. Where are the Lanthanides located? __________________________________________ 16. Where are the Actinides located? _____________________________________________ 17. Where are the Halogens located? _______________ ...
... 14. Where are the Transition Metals located? ______________________________________ 15. Where are the Lanthanides located? __________________________________________ 16. Where are the Actinides located? _____________________________________________ 17. Where are the Halogens located? _______________ ...
Date Period - Swift Classroom
... He put the elements in order by _______________________ He found that other properties such as _________________________, _______________________, and the ability to ______________________ with other elements seemed to ____________________ over and over. This repeating pattern is called ______ ...
... He put the elements in order by _______________________ He found that other properties such as _________________________, _______________________, and the ability to ______________________ with other elements seemed to ____________________ over and over. This repeating pattern is called ______ ...
ANSWERS-ATOMIC STRUCTURE WORKSHEET
... 5. A negative ion is (larger/smaller) than its parent atom. 6. A positive ion is (larger/smaller) than its parent atom. 7. As you go from left to right across a period, the first ionization energy generally (increases/decreases). Why? Increased positive nuclear charge, ENC increases, F of A increase ...
... 5. A negative ion is (larger/smaller) than its parent atom. 6. A positive ion is (larger/smaller) than its parent atom. 7. As you go from left to right across a period, the first ionization energy generally (increases/decreases). Why? Increased positive nuclear charge, ENC increases, F of A increase ...
of the periodic table
... Li, Na, K Proposed nature contained triads of elements. The middle element had properties that were an average of the other two members when ordered by the atomic weight. ...
... Li, Na, K Proposed nature contained triads of elements. The middle element had properties that were an average of the other two members when ordered by the atomic weight. ...
Chemistry test Review
... – Describes how many protons are in the nucleus of an atom – Also describes the number of electrons in a neutral atom ...
... – Describes how many protons are in the nucleus of an atom – Also describes the number of electrons in a neutral 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.