Results for "Liquid"

QHEM Chapter 14: Liquids and Solids

IMF's, Liquids and Solids, phase changes and Water

Q3_Lesson 3 - Properties of Liquids

Solids liquids Terms

Solids, Liquids, Gas IGCSE

INTERMOLECULAR FORCES AND PROPERTIES OF LIQUIDS

Chemistry Solids & Liquids

Chemical Calculations, Gases, Liquids, Solids, and Solutions

Conduction, Convection, et rayonnement Criteres Isolants et conducteurs Définition/processus de rayonnement, convection, et conduction Isolants et conducteurs Les conducteurs sont les choses qui facilement transfèrent l'énergie. Les plus populaires et utilisent conducteur est les métaux (cuivre, aluminium, or, argent etc.) Les isolants sont les choses qui réduisent/absorbent le flux (flow) de l'énergie, et sont utilisés pour la perte ou la gaine de chaleur. Les plus populaires et utilisés pour le chauffage sont du mousee, fibre, verre, et laine minérale. C’est quoi le rayonnement? Le rayonnement est une forme d'énergie, qui avance (travel) dans les vagues(sans particules) ou particules. Cela inclut des types d'énergie comme la lumière, la chaleur, qui produisent les rayons invisibles . La radiation peut être naturelle, comme celle du soleil, ou artificielle, comme traitements médicaux comme la radiothérapie. Particules relâcher (release) l'énergie quand en contact avec des chimiques, qui cause un réaction chimique, ou un température élevée. Quand cette énergie a été émise, elle voyage dans l’espace (space as in space in between one and another) et/ou à travers des matériaux. Par exemple, le rayonnement du soleil, avec une température très chaude, crée des rayonnements, qui se déplacent vers terre, et nous réchauffent. C’est quoi conduction? Conduction est le transfert d'énergie entre un matériau qui ont l'énergie, et un qui n’a pas. (Chaud et froid) Cet événement se déplace parce que l'énergie dans les particules de matière (the mouvement) se touche avec des autres particules d’autres matières, et quand touche transfèrent l'énergie. Par exemple, un pot avec des œufs. Le chaleur du feu qui chauffe le pot transfert un fraction d’énergie au pot, et le pot transfère une fraction de son énergie au les oeufs, et les oeufs cuits. C’est quoi convection? Convection est quand les particules dans un liquide/gaz qui sont chauffés, sont moins dense et se déplacent en haut parce qu'elles sont moins dense. Les particules froides coulant au bas, et se réchauffent, et devient moins dense, que créer un boucle (loop). En nature, le vent est un bon exemple de convection. Pendant le jour, le sol besoin/absorbent plus d'énergie du soleil que le mer/eau, donc l’air autour du terre s'élève place c’est plus chaud, et l’air plus froid de mer se déplacer pour remplacer l' espace vide, l’air du mer qui se déplace s'élève, et créer un boucle

1 What structures make up the gas exchange system in humans? Cartilage rings Trachea Bronchi Larynx Intercostal Muscles Alveoli Diaphragm Ribs Bronchioles Trachea: Moves air from outside the body to inside the lungs. Also called the windpipe Cartilage rings: C-shaped rings that hold open the trachea. Bronchi: The trachea splits into two bronchi, that lead into each lung. Bronchioles: The bronchi split into many smaller tubes that take air throughout the lungs. Ribs: Bones that protect the lungs from damage. Alveoli: At the ends of the bronchioles, where gas exchange takes place. Intercostal muscles: The muscle between the ribs. MHS Year 10 Science - BIOLOGY 2025 How does air, containing oxygen, get into and out of the lungs? Breathing in: Diaphragm contracts and moves down, intercostal muscles contract and move ribs up and out = more space in the chest = air moves in. Breathing out: Diaphragm relaxes and moves up, intercostal muscles relax and move ribs down and in = less space in the chest = air moves out. Carbon dioxide needs to be breathed out as it is toxic and will kill cells. Oxygen needs to be breathed in as it is needed by all cells to release energy from food (respiration) What structures make up the human circulatory system? The heart has 4 chambers, two atrium at the top and 2 ventricle at the bottom. There is a left and right side of the heart. The left side has thicker muscle than the right as it pumps blood a greater distance than the right side. The septum is the muscle between the two sides. There are 3 types of blood vessels. Arteries take blood away from the heart, veins that take blood towards the heart and very thin capillaries join the arteries and veins. Blood is made of a liquid called plasma and blood cells. There are three types of blood cells, red blood cells (carry oxygen) white blood cells (prevent disease) and platelets (form blood clots). 5 What does the heart look like? Aorta Right Vent sorrenated 3 Where does oxygen get into the blood? Air containing lots of oxygen is breathed in. The air travels down the trachea, bronchi, bronchioles to the alveoli. Gas exchange takes place in the alveoli. Oxygen is needed by all cells for respiration. Oxygen moves from the air in the alveoli into the blood in the capillaries surrounding the alveoli. Carbon dioxide is made during respiration and is toxic. It is removed from the blood as it travels past the alveoli. It is removed from the body when we breathe out

Skill III: Withdrawing Liquid from a Vial (15 minutes)

BUSINESS - 2.3.2 - LIQUIDITY

PROCEDURE #56: THICKENED LIQUIDS

Physics: Solids, Liquids and Gases - Unit 5

Lecture 48: Liquid dosage forms: Suspensions and emulsions 1

Lecture 47: Liquid dosage forms for oral administration- solutions

Solid Liquid Gases Quiz

Liquid, diet,EGD

Chapter 4 The Effects of Chemical Reactions. • Introduction to Chemical Reactions. - Chemical reaction: a process in which one or more substances change into one or more new substances. - Clues that a chemical reaction has occurred : 1. Color change Example: two colorless aqueous solutions mix together to produce a bright yellow precipitate. 2. A precipitate (solid) is formed when mixing two solutions together. 3. Gas formation. Bubbles of gas (effervescence) are produced when mixing substances together (solid – liquid or aqueous – aqueous ….) 4. Heat is produced. - Chemical reactions are described by using word equations or chemical equations. - Chemical equations need to be balanced when written because it shows the correct proportions (amounts) of chemicals in a reaction. - A balanced chemical equation has equal number of atoms of each element in the reactants (left hand side) and the products (right hand side). - Exercise: Balance the following equations. a) KClO3→KCl + O2 b) Na2O + H2O NaOH c) Cu + AgNO3 Cu(NO3)2 + Ag d) C3H7OH + O2 CO2 + H2O • Synthesis and Decomposition Reactions. Synthesis: Two or more substances (elements and / or compounds) combine to form one larger compound. General pattern: A + B → C Examples: N2 + 3 H2 → 2 NH3 CaO + CO2 → CaCO3 2 P + 3 Cl2 → 2 PCl3 Decomposition: This is opposite to synthesis; that is, one large compound breaks down (decomposes) into 2 or more simpler substances. Example: 2 KClO3 → 2 KCl + 3 O2 General pattern: R → S + T Remark: Usually decomposition happens due to heat or electricity. - Predicting the product of decomposition or synthesis reactions. 2 AlCl3 (s) → 2 Al (s) + 3 Cl2 (g) Zn (s) + S (s) → ZnS (s) 2 Zn (s) + O2 (g) → 2 ZnO(s) - Single Displacement (Replacement) Reactions. Definition: A reaction in which an element displaces (replaces) another element in a compound, producing a new compound and a new element. General pattern: A + BC → AC + B Example: Mg (s) + CuSO4 (aq) → MgSO4 (aq) + Cu (s) Zn (s) + 2 AgNO3 (aq) → Zn(NO3)2 (aq) + 2 Ag (s) Fe (s) + MgCl2 (aq) → no reaction. Remark: The element that displaces the other element in a compound must be more reactive (active) than that element, otherwise no reaction takes place. In the general pattern above, A should be more reactive than B for the reaction to proceed. The following reactivity (activity) series lists the chemical strength (reactivity) of the metals in order from the more reactive to the less reactive. KPlease stop calling my amazing zebra in the long Nahungry class. sorry !! Ca Mg Al Zn Fe Sn Pb H Cu Ag Examples of single displacement reactions : 2 Al (s) + 3 CuSO4 (aq) → Al2(SO4)3 (aq) + 3 Cu (s) Sn (s) + Zn(NO3)2 (aq) → no reaction Exercise: Complete and balance the following equations. If there is no reaction occurring write no reaction. a) 2 Al (s) + 6 HCl (aq) → 2 AlCl3 (aq) + 3 H2 (g) b) Cu (s) + H2SO4 (aq) → no reaction c) 2 AlCl3 (aq) + 3 Ca (s) → 3 CaCl2 (aq) + 2 Al (s) d) Mg (s) + 2 HNO3 (aq) → Mg(NO3)2 (aq) + H2(g) - Reactivity of halogens decreases down the group. F2> Cl2> Br2> I2 The reactions taking place for the halogens or their compounds are in solution (aqueous) Examples: Cl2 (aq) + 2 KBr (aq) → 2 KCl (aq) + Br2 (l) Cl2 (aq) + NaF (aq) → no reaction. Exercise: F2 (aq) + 2 LiCl (aq) → 2 LiF (aq) + Cl2 (g) I2 (aq) + NaCl (aq) → no reaction • Double displacement reactions. - Definition: A reaction in which two compounds mix together and an exchange of ions (elements) occurs which results in the formation of 2 new compounds. - General pattern: AB + CD → AD + CB - Solubility: the amount of solute that dissolves in a given amount of solvent at a given temperature. - When we say a substance is soluble, it means it dissolves in water; whereas if it is insoluble it means it doesn’t dissolve in water. - The compound in a reaction that is soluble is in aqueous (aq) phase, whereas the compound which is insoluble is in the solid state (s). - The solid which is formed in a double displacement reaction is called the precipitate and it is insoluble. - Solubility rules (used in double displacement reactions). 1. All alkali metal ions and ammonium ion (NH4+) are soluble. 2. All nitrates (NO3-) are soluble. 3. All sulfates (SO4-2) are solubleexceptwith Ba+2 , Pb+2 , Ca+2 , Sr+2 , Ag+ . 4. All chlorides, bromides and iodides(Cl-, Br-, I-) aresolubleexcept with Ag+ , Pb+2 , Hg+, Cu+ 5. All OH- are insolubleexceptwith rule 1, and Ba+2 and Sr+2 . 6. All oxides (O2-), sulfides (S2-), sulfites (SO32-), carbonates (CO32-), phosphates (PO43-) are insoluble except with rule 1 Remark: If all compounds formed in a double displacement reaction are soluble (aqueous) then no reaction takes place. Exercise: State whether each of the following compounds is soluble or insoluble ? Na2SO4 : Fe(NO3)2: LiOH: ZnSO4: PbBr2: BaSO4: Mg(OH)2: PbO: NH4Cl: Na2S: Cu(OH)2: KF: Exercise: Complete and balance the following chemical equations: - KNO3 (aq) + NaCl (aq) → - LiCl (aq) + AgNO3 (aq) → - Zn (s) + FeSO4 (aq) → - NaOH (aq) + CuCl2 (aq) → - ZnCl2 (aq) + Na3PO4 (aq) → - Pb(NO3)2 (aq) + K2S (aq) → • Net ionic equation: a chemical equation which shows ONLY the ions that are involved in the formation of the precipitate (solid). Examples: Pb+2 (aq) + S-2 (aq) → PbS (s) Ag+ (aq) + Cl- (aq) → AgCl (s) Cu+2 (aq) + 2 OH- (aq) → Cu(OH)2 (s) • Full ionic equation: an equation which shows All the ions in the soluble (aqueous compounds) in both reactants and products. Example: - 2 NaOH (aq) + CuCl2 (aq) → 2 NaCl (aq) + Cu(OH)2 (s) 2 Na+ (aq) + 2 OH- (aq) + Cu+2 (aq) + 2 Cl- (aq) → 2 Na+ (aq) + 2 Cl- (aq) + Cu(OH)2 (s) - 3 ZnCl2 (aq) + 2 Na3PO4 (aq) → Zn3(PO4)2 (s) + 6 NaCl (aq) Full ionicequation: 3 Zn+2(aq) + 6 Cl-(aq) + 6 Na+ (aq) + 2 PO4-3 (aq) → Zn3(PO4)2 (s) + 6 Na+ (aq) + 6 Cl- (aq) Net ionic equation: 3 Zn+2 (aq) + 2 PO4-3 (aq) → Zn3(PO4)2 (s) Exercise: Complete and balance the following equation, then write full ionic and net ionic equations for the reaction. Pb(NO3)2 (aq) + 2 NaI (aq) → Full ionic equation: Net ionic equation: Spectator ions: the ions that are not involved in the formation of the precipitate (solid). Note that the spectator ions appear on both sides of the full ionic equation. For example, in the above reaction, Na+ (sodium ions) and NO3- (nitrate ions) are the spectator ions. Exercise: Complete and balance the following equation, then write the net ionic equation and identify the spectator ions. BaCl2 (aq) + K2SO4 (aq) → Net ionic equation: Ba+2 (aq) + SO4-2 (aq) → Spectator ions: - Combustion reaction is a special type of (synthesis) reaction in which the substance reacts with (burns in) oxygen. Examples: C(s) + O2(g) → CO2(g) • Production of gases (lab scale): 1. CO2 2. SO2 3. H2 4. H2S (hydrogen sulfide) 5. NH3 (ammonia) General pattern of the chemical reactions to produce the above gases: 1. Metal carbonate + acid → CO2 Example: Na2CO3 (aq) + 2 HCl (aq) → 2 NaCl(aq) + CO2(g) + H2O(l) 2. Metal sulfite + acid → SO2 K2SO3 (aq) + 2 HCl (aq) → 2 KCl(aq) + SO2(g) + H2O(l) 3. Metal + acid → H2 Remark: This is a single displacement reaction therefore the metal used in the reaction should be higher in the reactivity series than hydrogen. Zn (s) + 2 HCl (aq) → ZnCl2 (aq) + H2(g) 4. Metal sulfide + acid → H2S Na2S (aq) + 2 HCl (aq) → 2 NaCl (aq) + H2S (g) 5. Ammonium compound + base (alkaline solution) → NH3 NH4Cl (aq) + NaOH (aq) → NaCl (aq) + NH3 (g) + H2O (l) Exercise: Write the net ionic equations for each of the above 5 reactions. Answers 1. 2 H+ (aq) + CO3-2(aq) → CO2(g) + H2O (l) 2. 2 H+ (aq) + SO3-2(aq) → SO2(g) + H2O (l) 3. Zn(s) + 2 H+(aq) → Zn+2(aq) + H2(g) 4. 2H+ (aq) + S-2 (aq) → H2S (g)

Laboratory Operations- liquid liquid extractions