Chem class(22apr)
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This document discusses the physical and chemical properties of group 1 elements on the periodic table, also known as alkali metals. Physically, they are soft metals with silvery surfaces that conduct heat and electricity well. Chemically, they become more reactive down the group due to increasing atomic size and decreasing attraction of the nucleus. Their reactivity makes them burn vigorously in reactions with oxygen, water, and halogens like chlorine.
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1) It describes how Dmitri Mendeleev developed the first periodic table by ordering elements by atomic mass and identifying patterns in their properties, allowing him to predict undiscovered elements.
2) The main features of the periodic table are described, including groups (columns) and periods (rows) arranged by increasing atomic number.
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The document discusses various chemical groups and families, including their properties and common uses. It covers the alkali metals, alkaline earth metals, transition metals, inner transition metals (lanthanides and actinides), and other nonmetal groups such as carbon, nitrogen, oxygen, halogens, noble gases, and hydrogen. For each group, it highlights some of the most abundant elements, their physical and chemical characteristics, and important commercial applications.
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The document discusses the periodic table and properties of different families of elements. It describes five main families: alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. For each family it provides examples of elements in that family and discusses their common chemical and physical properties, such as reactivity, state of matter, conductivity, and how they are found in nature.
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Group 18 consists of helium, neon, argon, krypton, xenon, and oganesson. Noble gases have full outer electron shells, making them chemically inert. Their melting and boiling points increase down the group as atomic size increases and van der Waals forces strengthen.
Group 1 includes lithium, sodium, potassium, cesium, and francium. Alkali metals react by losing one electron to form stable ions. Reactivity increases down the group as the valence electron is more loosely held. They react with water to form hydroxides and oxygen to form ox
Chemistry of Alkali Metals MANIK
Chemistry of alkali and alkaline earth metals and halogen compounds including their
Pharmaceutical applications.
GCSE Chemistry [C3]
The document provides information on the structure of atoms, ionic and covalent bonding, the periodic table, properties of metals and non-metals, and chemical reactions. It discusses how atoms are composed of protons, neutrons and electrons, and how electrons are arranged in shells. It also explains how ionic bonding occurs through transfer of electrons between metals and non-metals, while covalent bonding involves sharing of electrons between non-metals.
Group i elements
The document discusses the properties of Group 1 elements (alkali metals) on the periodic table. Some key points:
1) The alkali metals have a general electronic configuration of ns1 and include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), and cesium (Cs).
2) Their physical properties, such as atomic radius and ionization energy, decrease down the group as nuclear charge decreases due to the lanthanide contraction.
3) Their chemical properties include reacting vigorously with water to form alkaline hydroxides and oxygen to form oxides/peroxides/superoxides. They are highly reactive metals.
IB Chemistry on Reactivity Series vs Electrochemical Series
This document provides a tutorial on the reactivity series versus the electrochemical series.
The reactivity series orders metals based on their reactivity in reactions like with water or acids. It finds potassium to be the most reactive, followed by sodium then lithium.
The electrochemical series orders metals based on their standard electrode potentials, a thermodynamic measurement of their tendency to gain or lose electrons. It finds lithium to have the most negative potential, making it the best reducing agent and the least likely to gain electrons.
There is a correlation between the two series but not a perfect match. Kinetics factors like activation energy can cause differences, making potassium more reactive with water even though lithium is higher in
Periodic Table Families Revised 09
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IB Chemistry on Reactivity Series vs Electrochemical Series
The document discusses the reactivity and electrochemical series of group 1 alkali metals lithium, sodium, and potassium. While lithium has the most negative standard reduction potential, indicating it is most easily oxidized, potassium is the most reactive when reacting with water and acids due to lower kinetic barriers. The electrochemical series is a thermodynamic measurement based on standard potentials, while the reactivity series considers reaction kinetics. Thus, there is a correlation but not perfect agreement between the two series.
material science digital assignment
1. The Young's moduli of alkali metals are given below in units of GN m-1: Li
(11.5), Na (9.0), K (3.5), Rb (2.7), Cs (1.8) and Fr (1.7). Compare this with the
corresponding values of the melting points. Give a reason for this sequence.
Periodicity
The document provides information about trends in the periodic table including:
- Atomic radius decreases and electro-negativity increases when going left to right or down groups 1 and 7 due to increased shielding and decreased pull from protons.
- Metalloids are between metals and non-metals. Metals have properties like conductivity while non-metals want to gain electrons. Noble gases do not react.
- The periodic table was created by Dmitri Mendeleev to show patterns in properties based on atomic mass.
S-Block Elements
This document discusses the characteristic properties of s-block elements, which include the alkali metals (Group IA) and alkaline earth metals (Group IIA). Some key points discussed include:
- S-block elements have their outermost shell electrons in the s orbital.
- Alkali metals react vigorously with water to form alkaline hydroxides and hydrogen gas. Reactivity increases down the group.
- They form oxides, peroxides, and superoxides with oxygen. Oxidation states include -2, -1, and -1/2.
- Properties such as ionization energy, hydration energy, and metallic character generally decrease or increase moving down a group and across a period,
Chemistry of alkali and alkaline earth metals and halogen compounds MANIK
Chemistry of alkali and alkaline earth metals and halogen compounds including their Pharmaceutical applications.
2. group 1
The document discusses the chemical properties of alkali metals. It explains that alkali metals react vigorously with oxygen and water. The reactivity increases down the group as the atoms get larger, shielding the outer electrons from the nucleus and making them easier to lose. Equations for reactions of lithium, sodium, and potassium with oxygen, water, and other substances are provided. Flame tests for group 2 metals are also discussed.
Replacement reactions
This document discusses 5 common types of chemical reactions: replacement, combination, combustion, decomposition, and exchange reactions. It provides examples of each type of reaction and discusses how to identify them based on the reactants and products. Key signs of chemical reactions are also outlined, including changes in color, temperature, production of gases or solids, pH, and smell. The document also introduces activity series for metals and nonmetals, which can be used to predict whether replacement reactions will occur based on the reactivity of the elements involved.
Group IA.pdf
The document summarizes the properties and reactivity of alkali metals. It discusses their physical properties including softness, low density, and good heat and electricity conductivity. It describes their chemical reactivity including reactions with oxygen, halogens, nitrogen, carbon, and water. Alkali metals readily lose their outer shell electron to form +1 ions. Their reactivity increases down the group as atomic size increases. Common compounds include oxides, hydroxides, peroxides, and superoxides. Sodium and potassium are the most abundant in nature while lithium, rubidium, and cesium are rarer.
Properties of metals slides
The document describes various properties of metals. It discusses the physical properties of metals, including their high melting and boiling points, malleability, ductility, and ability to conduct heat and electricity well. It also describes alloys as mixtures of metals that are stronger than pure metals. Additionally, the document outlines some chemical properties of metals, such as their reactivity patterns and reactions with water, steam, and acids according to the reactivity series. It provides examples of equations to represent these reactions.
Active series of metal
The document discusses the activity series of metals and how it can be used to predict products of displacement reactions. It provides examples of reactions that can occur between different metals and solutions like aluminum displacing hydrogen from acid, sodium displacing hydrogen from water, and magnesium displacing zinc from a solution. The document then describes a procedure for developing an activity series based on laboratory observations of reactions between metal strips and salt solutions. Observations such as gas evolution, color changes, and precipitate formation are noted. The results are recorded in a table showing reactions between various metals and solutions of salts like aluminum sulfate, copper sulfate, zinc sulfate, nickel sulfate, lead sulfate, and iron sulfate.
Chem 101 week 6 pt2
This document contains lecture notes on quantitative analysis in chemistry. It discusses gravimetric analysis, which determines the amount of a substance by converting it into a product that can be isolated and weighed. An example is given of determining the amount of lead in water by precipitating lead sulfate, filtering and weighing the precipitate. A practice problem demonstrates calculating the mass of lead from the mass of lead sulfate precipitate obtained.
12.-s-block-notes.pdf
1. The document discusses the properties and reactions of alkali metals, which have an ns1 electronic configuration and are highly reactive metals.
2. It describes their physical properties including large atomic size, low ionization energy, and increasing reactivity down the group from Li to Cs.
3. The chemical properties discussed include forming ionic compounds such as oxides, hydroxides, halides and reacting vigorously with water and acids.
908_Ch 11 Alkali metals.pptx
The document discusses the group 1 elements known as the alkali metals (lithium, sodium, potassium, rubidium, cesium, and francium). It describes their physical and chemical properties, including their low melting points, softness, and reactivity with air and water. It also discusses the industrial extraction and important commercial uses of several alkali metals and their compounds, such as in batteries, fertilizers, soaps, and other products. The solubility and hydration of alkali metal salts is influenced by factors like the ions' charge densities.
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IB Chemistry on Reactivity Series vs Electrochemical Series
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Chem class(22apr)
- 1. H He Little Belly Boy Come Near Oreo For Nutrition Naughty Man And Silly People Should Consume A lot of Kentucky Combo
- 3. Group 1 elements are alkaline, Call them as Alkali metals.
- 5. Physical properties of group 1 elements soft metals silvery and shiny surfaces low melting and boiling points good conductors of heat and electricity low density
- 6. When down the group 1…. 1. Hardness 2. Atomic size the number of atomic shell ↑ 3. melting point and boiling point atomic size ↑ distance between the nucleus and the valance electron shell ↑ metallic bond between atoms ↓ 4. Density Size ↑ mass more than increase in volume atoms are closer
- 7. Element Radius M.p B.p Hardness Density Electro- positivity Li Na K Rb Cs Fr decrease increase
- 9. x x x x x 3 P 3 e 3 P 2 e 3 + 2 - 1 + Duplet (stable) Li - 1e → Li+
- 10. x xx xx x x xxxx xx xx x x xxxx 11 P 11 e 11 P 10 e 11 + 10 - Na - 1e → Na+ Octet (stable) 1 +
- 11. K - 1e → K+
- 12. Electropositivity Increase(↑) down the group. The tendency to donate electrons to form positive ions x xx xx x x xxxx x x Li Na x
- 13. Down the group 1, Reactivity ↑ Atomic size ↑ The 1 valence electron become far from the nucleus. The force of attraction of nucleus on the valence ↓ The single electron becomes easier to be release. Reactivity ↑ Li < Na < K < Rb < Cs < Fr
- 14. 3 reactions in group 1 With Oxygen With water With halogens
- 16. Reaction with oxygen Alkali metals + oxygen alkali metal oxides Ex: 4 Li(s) + O2(g) 2Li2O(s)
- 18. metal reaction Phenolphthalein indicator Li Burn with a red flame. Turns pink Na Burn with a bright yellow flame. Turns pink K Burn violently with a very bright purplish flame. Turns pink Reactivity ↑ down the group
- 20. Reaction with water Alkali metals + water alkaline metals hydroxide + hydrogen gas Ex: 2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)
- 21. met al reaction Phenolphthal ein indicator Li Move slowly on the water surface. Turns pink Na Move at a fast speed on water surface with a “hissing” sound, burn with yellow flame. Turns pink K Move very fast speed and burn with a purple flame. Turns pink Reactivity ↑ down the group
- 22. Reaction with Halogen Chlorine gas
- 23. Reaction with Halogen Alkali metals + halide alkali metals halide Ex: 2K(s) + Cl2(g) 2KCl(s)
- 24. metal reaction product Li Burn slowly with a reddish flame. White solid is obtained Na Burn brightly with a yellowish flame. White solid is obtained K Burn very brightly with purplish flame. White solid is obtained Reactivity ↑ down the group
- 25. Safety Precautions Alkali metals are highly reactive to water and air. Kept under non-reactive oil (eg. Paraffin oil) Never handle with your fingers.
- 26. Summary: Physical • Shiny and silvery surface • conductors of heat and electricity • Hardness • Atomic size • Mp • Bp • density Chemical • Electropositivity • Reactivity: • Reaction with oxygen • Reaction with water • Reaction with chlorine