unit 3 ppt
... discovered new elements and, in more recent years, synthesized new ones in the laboratory. Each of the more than 40 new elements, however, can be placed in a group of other elements with similar properties. The periodic table is an arrangement of the elements in order of their atomic numbers so that ...
... discovered new elements and, in more recent years, synthesized new ones in the laboratory. Each of the more than 40 new elements, however, can be placed in a group of other elements with similar properties. The periodic table is an arrangement of the elements in order of their atomic numbers so that ...
Atoms, Elements, and the Periodic Table Spring Packet
... d. noble gas ____ 8. B, boron, 5 ____ 9. W, tungsten, 74 ____ 10. Rh, rhodium, 45 ____ 11. Ne, neon, 10 Complete each statement. 12. Chlorine-35 and chlorine-37 have a different number of ____________________. 13. The likely location of the negatively charged particles in an atom is called a(n) ____ ...
... d. noble gas ____ 8. B, boron, 5 ____ 9. W, tungsten, 74 ____ 10. Rh, rhodium, 45 ____ 11. Ne, neon, 10 Complete each statement. 12. Chlorine-35 and chlorine-37 have a different number of ____________________. 13. The likely location of the negatively charged particles in an atom is called a(n) ____ ...
The Periodic Table
... 3. The elements that border either side of the zigzagged line are metalloids. Metalloids have properties of both metals and nonmetals. Name two metalloids. 4. The alkali metals are in group 1. They have only one electron in their outer shell. They are very reactive and have a low melting point. Shad ...
... 3. The elements that border either side of the zigzagged line are metalloids. Metalloids have properties of both metals and nonmetals. Name two metalloids. 4. The alkali metals are in group 1. They have only one electron in their outer shell. They are very reactive and have a low melting point. Shad ...
How the Periodic Table Works
... Alkaline earth metals (group 2 or IIA) include magnesium, calcium and barium among others. These elements have two valence electrons, which they yield in chemical reactions. Although they're less reactive than alkali metals, they're not usually found alone in nature. For example, calcium combines wi ...
... Alkaline earth metals (group 2 or IIA) include magnesium, calcium and barium among others. These elements have two valence electrons, which they yield in chemical reactions. Although they're less reactive than alkali metals, they're not usually found alone in nature. For example, calcium combines wi ...
Name Pre-Test : Atomic Structure and the Periodic Table
... 9. Group 1 includes the alkaline metals. What are the general properties of elements in this group? 10. Between groups 2 and 3 are the transition metals. a. Describe the general properties of the transition metals. b. List three examples of transition metals and their uses. 11. Group 14 is called th ...
... 9. Group 1 includes the alkaline metals. What are the general properties of elements in this group? 10. Between groups 2 and 3 are the transition metals. a. Describe the general properties of the transition metals. b. List three examples of transition metals and their uses. 11. Group 14 is called th ...
File
... In this lesson you will learn how to describe periodic trends in electronegativity, melting point and boiling point VOCABULARY electronegativity DO NOW (Answer the following questions by using your textbook) ...
... In this lesson you will learn how to describe periodic trends in electronegativity, melting point and boiling point VOCABULARY electronegativity DO NOW (Answer the following questions by using your textbook) ...
Elements and Atoms: The Building Blocks of Matter
... The human body is composed of elements, the most abundant of which are oxygen (O), carbon (C), hydrogen (H) and nitrogen (N). You obtain these elements from the foods you eat and the air you breathe. The smallest unit of an element that retains all of the properties of that element is an atom. But, ...
... The human body is composed of elements, the most abundant of which are oxygen (O), carbon (C), hydrogen (H) and nitrogen (N). You obtain these elements from the foods you eat and the air you breathe. The smallest unit of an element that retains all of the properties of that element is an atom. But, ...
VIBRATIONS AND WAVES
... move left-to-right across a period. The increased nuclear charge of each successive element produces an increased hold on the valence electrons. The first ionization energies generally decrease as you move down a group. Because atomic size increases down a group, the valence electrons are farther fr ...
... move left-to-right across a period. The increased nuclear charge of each successive element produces an increased hold on the valence electrons. The first ionization energies generally decrease as you move down a group. Because atomic size increases down a group, the valence electrons are farther fr ...
The Periodic Table - Prairie Rose School Division No. 8
... Patterns: reactivity of metals What happens to the reactivity of metals along a period? What happens to the reactivity of metals down a group? ...
... Patterns: reactivity of metals What happens to the reactivity of metals along a period? What happens to the reactivity of metals down a group? ...
KS4 The Periodic Table 3548KB
... Patterns: reactivity of metals What happens to the reactivity of metals along a period? What happens to the reactivity of metals down a group? ...
... Patterns: reactivity of metals What happens to the reactivity of metals along a period? What happens to the reactivity of metals down a group? ...
KS4 Chemistry The Periodic Table 1 of 47 © Boardworks Ltd 2005
... Patterns: reactivity of metals What happens to the reactivity of metals along a period? What happens to the reactivity of metals down a group? ...
... Patterns: reactivity of metals What happens to the reactivity of metals along a period? What happens to the reactivity of metals down a group? ...
AP Chemistry Chapter 7 Lecture Notes 7.1 Development
... •The larger the ionization energy, the more difficult it is to remove the electron. •There is a sharp increase in ionization energy when a core electron is removed. Variations in Successive Ionization Energies •Ionization energies for an element increase in magnitude as successive electrons are remo ...
... •The larger the ionization energy, the more difficult it is to remove the electron. •There is a sharp increase in ionization energy when a core electron is removed. Variations in Successive Ionization Energies •Ionization energies for an element increase in magnitude as successive electrons are remo ...
chemical bonds: the formation of compounds from atoms
... A sodium atom is larger than a silicon atom. Sodium and silicon are both in period 3. Going across a period, the radii of atoms decrease. A bromide ion is larger than a potassium ion. The bromide ion has 35 protons and 36 electrons, creating a charge imbalance that results in a lessening of the attr ...
... A sodium atom is larger than a silicon atom. Sodium and silicon are both in period 3. Going across a period, the radii of atoms decrease. A bromide ion is larger than a potassium ion. The bromide ion has 35 protons and 36 electrons, creating a charge imbalance that results in a lessening of the attr ...
Chapter 11
... A sodium atom is larger than a silicon atom. Sodium and silicon are both in period 3. Going across a period, the radii of atoms decrease. A bromide ion is larger than a potassium ion. The bromide ion has 35 protons and 36 electrons, creating a charge imbalance that results in a lessening of the attr ...
... A sodium atom is larger than a silicon atom. Sodium and silicon are both in period 3. Going across a period, the radii of atoms decrease. A bromide ion is larger than a potassium ion. The bromide ion has 35 protons and 36 electrons, creating a charge imbalance that results in a lessening of the attr ...
Chem.-Chapter-6-notes
... left to right across a period. Cations are always smaller than the atoms from which they form. Anions are always larger than the atoms from which they form. In general, electronegativity values decrease from top to bottom within a group. For representative elements, the values tend to increase from ...
... left to right across a period. Cations are always smaller than the atoms from which they form. Anions are always larger than the atoms from which they form. In general, electronegativity values decrease from top to bottom within a group. For representative elements, the values tend to increase from ...
Group 16: The Oxygen Family - Chemwiki
... Sulfur also exhibits a wide range of oxidation states, with values ranging from -2 to +6. It is often the central ion in a compound and can easily bond with up to 6 atoms. In the presence of hydrogen it forms the compound hydrogen sulfide, H2S, a poisonous gas incapable of forming hydrogen bonds and ...
... Sulfur also exhibits a wide range of oxidation states, with values ranging from -2 to +6. It is often the central ion in a compound and can easily bond with up to 6 atoms. In the presence of hydrogen it forms the compound hydrogen sulfide, H2S, a poisonous gas incapable of forming hydrogen bonds and ...
11. Patterns in the Periodic Table
... Where were the elements made? There are 92 naturally-occurring elements and about 15 artificially-produced elements. Elements were originally made in stars. In the early stages of a star’s life, light elements, such as hydrogen and helium, are formed. These fused together to make heavier elements s ...
... Where were the elements made? There are 92 naturally-occurring elements and about 15 artificially-produced elements. Elements were originally made in stars. In the early stages of a star’s life, light elements, such as hydrogen and helium, are formed. These fused together to make heavier elements s ...
11. Patterns in the Periodic Table
... Where were the elements made? There are 92 naturally-occurring elements and about 15 artificially-produced elements. Elements were originally made in stars. In the early stages of a star’s life, light elements, such as hydrogen and helium, are formed. These fused together to make heavier elements s ...
... Where were the elements made? There are 92 naturally-occurring elements and about 15 artificially-produced elements. Elements were originally made in stars. In the early stages of a star’s life, light elements, such as hydrogen and helium, are formed. These fused together to make heavier elements s ...
File - eScience@Kings
... Where were the elements made? There are 92 naturally-occurring elements and about 15 artificially-produced elements. Elements were originally made in stars. In the early stages of a star’s life, light elements, such as hydrogen and helium, are formed. These fused together to make heavier elements s ...
... Where were the elements made? There are 92 naturally-occurring elements and about 15 artificially-produced elements. Elements were originally made in stars. In the early stages of a star’s life, light elements, such as hydrogen and helium, are formed. These fused together to make heavier elements s ...
Document
... They also have higher melting points. They are less reactive than alkali metals, but they too are too reactive to be found free in nature. ...
... They also have higher melting points. They are less reactive than alkali metals, but they too are too reactive to be found free in nature. ...
Page 8: Review 1
... List the early attempts of classification of the elements. Match scientists and their contributions to the development of the P.T. State the modern periodic law. Distinguish groups and periods in the P.T. Define chemical stability using the octet rule. Use the periodic table to predict electron conf ...
... List the early attempts of classification of the elements. Match scientists and their contributions to the development of the P.T. State the modern periodic law. Distinguish groups and periods in the P.T. Define chemical stability using the octet rule. Use the periodic table to predict electron conf ...
C1 - Powerpoint - tonyconnett.com
... 1. What happens to the boiling point of the metals as you move down group 1 2. Group 1 atoms want to loose an electron, do you think it would be easier to remove an electron from Lithium or Cs? 3. What is the most reactive element in group 1? 4. Group 7 atoms want to gain an electron, which atom wou ...
... 1. What happens to the boiling point of the metals as you move down group 1 2. Group 1 atoms want to loose an electron, do you think it would be easier to remove an electron from Lithium or Cs? 3. What is the most reactive element in group 1? 4. Group 7 atoms want to gain an electron, which atom wou ...
7.1 The Periodic Table
... • Physical properties include color, texture, density, brittleness, and state (solid, liquid, or gas). • Melting point, boiling point, and specific heat are also physical properties. ...
... • Physical properties include color, texture, density, brittleness, and state (solid, liquid, or gas). • Melting point, boiling point, and specific heat are also physical properties. ...
d) Ramsay. The idea of arranging the elements in the periodic table
... The group of soft, silvery active metals, all of which have one electron in an s orbital, is known as the a) alkaline-earth metals. b) transition metals. c) alkali metals. ...
... The group of soft, silvery active metals, all of which have one electron in an s orbital, is known as the a) alkaline-earth metals. b) transition metals. c) alkali metals. ...
Periodicity of Elements
... Using an activity series, what can you deduce about the relationship between electron affinity and reactivity of nonmetals? Explain in 3-4 paragraphs the organization and usefulness of the modern periodic table based on what you have learned in class and what you have learned from this activity. ...
... Using an activity series, what can you deduce about the relationship between electron affinity and reactivity of nonmetals? Explain in 3-4 paragraphs the organization and usefulness of the modern periodic table based on what you have learned in class and what you have learned from this activity. ...
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.