Kemi 7-9, del 3: Neutralisation och salter

Kemi 7-9, del 3

• Neutralisation: Mixing equal amounts of acid and alkali.
• Neutralisation product: Salt and water.
• Evaporation: Leaving behind a solid salt if water evaporates from a solution.
• Salt production methods: Three ways to make salts.
• Magnesium in acid: Magnesium reacting with acid produces magnesium salts and hydrogen gas.
• Salt alternative names: Common salt is also known as sodium chloride or table salt.
• De-icing: Adding salt to ice lowers its freezing point.
• Calcium carbonate: A natural compound found in limestone, chalk, and marble. Used in construction materials.
• Gypsum: Calcium sulfate (CaSO4).
• Salmiak: Ammonium chloride (NH4Cl).
• Salpeter uses: Used in fertilizers, explosives, and other industrial applications.
• Electrical conductivity: Solid salts do not conduct electricity but liquid or dissolved salts do.
• Oxid examples: List of chemical formulas representing oxides that are not ionic compounds.
• Metallic component: Aluminum is a metal found in gemstones like sapphires, rubies, and emeralds.

Kemi 7-9, del 3 - sid 2

• Noble gases: Elements with filled outer electron shells.
• Electron shell attainment: How atoms achieve a stable electron configuration, either by gaining or losing electrons.
• Atoms vs. ions: Differences between electrically neutral atoms and charged ions.
• Positive ions examples: Examples of positive ions, written with corresponding chemical formulas.
• Negative ions examples: Examples of negative ions, written with corresponding chemical formulas.
• Magnesium to magnesium ion: Explanation of how magnesium becomes an ion.
• Compound ion examples: Examples of negatively and positively charged compounds.
• Simple ion examples: Examples of individual charged atoms.
• Ion bonding: Explanation of ionic bonding.
• Ionic compound examples: Explanation of a compound formed by ionic bonding.
• Metallic ions examples: Examples of metal ions.
• Compound anion examples: Examples of negatively charged compounds.

Kemi 7-9, del 3 - sid 3

• Periodic table elements: List of chemical elements with symbols.
• Periodic table gas formation: Explanation of how gases are placed on the periodic table.
• Elements state of matter: List of elements that are liquid or gas at room temperature.
• Atomic number relations: Elements with atomic numbers and their relationship.
• Electronic configuration of elements: Explanation of how elements contain electrons.
• Electron shells of elements: Explanation of how elements are linked, considering electrons.
• Elements by group: List of elements by group, considering electrons.
• Valence electrons by Group: Explanation of the number of valence electrons in different groups.
• Element valence electrons examples: Examples of how to identify valence electrons from a periodic table.

Kemi 7-9, del 3 - sid 4

• Periodic table creator: Dmitri Mendeleev.
• Period commonality: The same number of electron shells.
• Group name: Column.
• Group similarity: Similar properties due to same valence electron configuration.
• Metallic families: Names of families of metals.
• Valence electrons in metals: Usually 1-3 valence electrons.
• Metalloids characteristics: Transitional properties in between metals and nonmetals.
• Valence electrons in alkali metals: One valence electron.
• Alkali metals reactions: React with water to form alkaline solutions.
• Halogens reactions: React readily with metals and other elements.
• Inert gas reactions: Generally do not react with other elements due to stable electron configuration.
• Transition metals properties: Varied properties like high melting points and variable oxidation states.
• Chemical bonding definitions: Description of chemical interactions between atoms involving electron sharing.
• Molecular compounds: Explanation of compounds formed by covalent bonds.

Kemi 7-9, del 3 - sid 5

• Atomic model developer: J.J. Thomson's contribution to the atomic model.
• Electron shell developer: Niels Bohr developed the model of electrons in shells.
• Subatomic particle charges: Proton (+) and neutron (neutral) are in the nucleus. Electron (-).
• Nucleus components: Protons and neutrons.
• Determining elements: Atomic number defines an element.
• Valence electrons significance: Key to chemical reactivity.
• Mass number definition: Total number of protons and neutrons.
• Isotopes meaning: Atoms of the same element with different number of neutrons.
• Atom stability: Different from stable or radioactive.
• Drawing atoms and atoms with shells: Explanation of how to sketch atoms with electron distribution in shells.

Kemi 7-9, del 3 - sid 6

• Electron shell levels: Explanation of electron shells and their maximum capacity for electrons.
• Elements and Atomic number: Identification of elements and corresponding atomic numbers.
• Electronic configuration: Description of the electron arrangement of different elements.
• Element groups and periods: Categorization of elements into groups according to their electronic configurations.
• Group properties and periods: Explanation of similar properties in groups and gradual changes in properties across periods.
• Periods and electronic configuration: Explanation of how electronic configuration changes within a period and correlates to properties.
• Electron shell names: Names of electronic shells.
• Electron numbers per shell: Maximum capacity of different shells.
• Identifying and writing element names: Examples of how to list, write chemical names, elements, and atomic symbols.

Kemi 7-9, del 3 - sid 7

• Alkalimetals examples: Li, Na, K.
• Alkalimetals reactivity reason: Low ionization energy, readily lose electrons.
• Alkali metals characteristics: Soft, silvery, very reactive.
• Hallogen families: Examples F, Cl, Br, I.
• High electronegativity: Tendency to attract electrons.
• Inert gases descriptions: Stable outer electron shells (full electron shells).
• Inert gases reactivity: Very low reactivity, very stable.
• Gases in lightbulbs: Use of inert gas (like argon) to prevent filament from burning.
• Atoms reaching stability: Explanation of how different atoms attain stable configurations through chemical bonds.
• Different atomic bond types: Description of covalent, ionic, and metallic bonds.
• Water molecule structure: Simple diagram of a water molecule.

Kemi 7-9, del 3 - sid 8

• Opposite charges: Attracting charges in ionic bonding.
• Ionic formula examples: Combination of positively and negatively charged ions.
• Chemical formula types: Description of different chemical formulas for reactions and compounds.
• Chemical reactions principles: Explanation of the necessity of equal amounts of atoms on both sides of chemical equations.
• Basic chemical reactions: Chemical reactions for different compounds.
• Balancing chemical formulas: How to ensure correct atomic count on both sides of reaction equations.

Detta quiz handlar om neutralisation, saltproduktion och olika typer av salter. Lär dig om reaktioner med magnesium och hur salter används, inklusive deras användning inom bygg och industri. Testa din kunskap om kemiska processer och salters egenskaper.