Problem Set 2
... Then indicate: a) The oxidation step: ----------------------------------------------------b) The reduction step: ------------------------------------------------------c) The oxidizing agent: ------------------------------------------------------d) The reducing agent: -------------------------------- ...
... Then indicate: a) The oxidation step: ----------------------------------------------------b) The reduction step: ------------------------------------------------------c) The oxidizing agent: ------------------------------------------------------d) The reducing agent: -------------------------------- ...
Ionic Bonding
... 13. How many elements are there in a tertiary compound? 14. Use each of the following terms correctly in a sentence about the formation of compounds: (a) polyatomic ion (b) oxyanion (c) hydrate 15. Write the IUPAC name for each of the following ionic compounds: (a) NaNO3(s) (found in tobacco) (b) Na ...
... 13. How many elements are there in a tertiary compound? 14. Use each of the following terms correctly in a sentence about the formation of compounds: (a) polyatomic ion (b) oxyanion (c) hydrate 15. Write the IUPAC name for each of the following ionic compounds: (a) NaNO3(s) (found in tobacco) (b) Na ...
Unit 9 The p-Block Elements
... E.A. = ∆H0 Electron affinity decreases numerically with increasing atomic number. This is because the outer electrons become more shielded from the nucleus as the atomic size increases, so the tendency to attract another electron decreases as the group is descended. (d) Suggest a reason why the elec ...
... E.A. = ∆H0 Electron affinity decreases numerically with increasing atomic number. This is because the outer electrons become more shielded from the nucleus as the atomic size increases, so the tendency to attract another electron decreases as the group is descended. (d) Suggest a reason why the elec ...
Unit 3 Practice Test
... A. Non-metals generally have the higher electronegativities and tend to attract electrons to themselves in a chemical bond. B. Elements with high ionization energies tend to have small atomic radii. C. Elements with high electronegativities generally form ions with small radii. D. The second ionizat ...
... A. Non-metals generally have the higher electronegativities and tend to attract electrons to themselves in a chemical bond. B. Elements with high ionization energies tend to have small atomic radii. C. Elements with high electronegativities generally form ions with small radii. D. The second ionizat ...
View Article - Asian Journal of Chemistry
... extracted with ethyl acetate (20 mL × 3) and the combined organic layer was dried over sodium sulfate, filtered and concentrated by vacuum distillation. The resulting compound was characterized by IR, 1H NMR. IR (KBr, νmax, cm-1): 2982 s, 2892 s, 1741 s, 1443 m, 1372 m, 1336 s, 1225 s, 1158 s, 1063 ...
... extracted with ethyl acetate (20 mL × 3) and the combined organic layer was dried over sodium sulfate, filtered and concentrated by vacuum distillation. The resulting compound was characterized by IR, 1H NMR. IR (KBr, νmax, cm-1): 2982 s, 2892 s, 1741 s, 1443 m, 1372 m, 1336 s, 1225 s, 1158 s, 1063 ...
PERIODIC TABLE
... 40- When (C8H16) is burned in oxygen atmosphere, we obtain (CO2) and (H2O) according to the following equation: a C8H16 + b O2 → c CO2 + d H2O In a balanced equation, the factors a, b, c, and d have the values: a- (a = 1, b = 1, c = 1, d = 1) b- (a = 1, b = 12, c = 8, d = 16) c- (a = 1, b = 12, c = ...
... 40- When (C8H16) is burned in oxygen atmosphere, we obtain (CO2) and (H2O) according to the following equation: a C8H16 + b O2 → c CO2 + d H2O In a balanced equation, the factors a, b, c, and d have the values: a- (a = 1, b = 1, c = 1, d = 1) b- (a = 1, b = 12, c = 8, d = 16) c- (a = 1, b = 12, c = ...
File
... halogens? All halogens have seven electrons in their outer shell. This means that: They can easily obtain a full outer shell by gaining one electron. They all gain an electron in reactions to form negative ions with a -1 charge. ...
... halogens? All halogens have seven electrons in their outer shell. This means that: They can easily obtain a full outer shell by gaining one electron. They all gain an electron in reactions to form negative ions with a -1 charge. ...
The Periodic Table of Elements
... therefore it becomes more difficult for the nucleus to attract an electron to form an ion most reactive is fluorine; least reactive is iodine all halogens form ions with single negative charge eg F-, Cl-, BrExists as diatomic molecules eg F2, Cl2, Br2, I2 reacts vigorously with metals to form ioni ...
... therefore it becomes more difficult for the nucleus to attract an electron to form an ion most reactive is fluorine; least reactive is iodine all halogens form ions with single negative charge eg F-, Cl-, BrExists as diatomic molecules eg F2, Cl2, Br2, I2 reacts vigorously with metals to form ioni ...
specimen
... ‘Dot-and-cross’ diagrams are used to model which electrons are present in the ion. Draw a ‘dot-and-cross’ diagram, including outer electron shells only, to show the ions present in magnesium chloride, MgCl2. ...
... ‘Dot-and-cross’ diagrams are used to model which electrons are present in the ion. Draw a ‘dot-and-cross’ diagram, including outer electron shells only, to show the ions present in magnesium chloride, MgCl2. ...
CHM 212 - The Federal University of Agriculture, Abeokuta
... with increasing relative molar mass. 4. They are all coloured, the depth of the colour increasing with increase in atomic number. Fluorine=pale yellow Chlorine=pale green Bromine=red brown Iodine=Shiny black 5. All halogens except fluorine dissolve slightly in water and colour it. Fluorine is a stro ...
... with increasing relative molar mass. 4. They are all coloured, the depth of the colour increasing with increase in atomic number. Fluorine=pale yellow Chlorine=pale green Bromine=red brown Iodine=Shiny black 5. All halogens except fluorine dissolve slightly in water and colour it. Fluorine is a stro ...
Metals and non-metals III IMPORTANT POINTS Non-metals
... 1. a. Magnesium, chromium and sodium are all metals, hence, they react with oxygen to form basic oxides b. Chromium, as it is a transition metal. Metals have high density and coloured compounds are formed by transition metals. c. Bromine - the formula is Br2, that is, two atoms of bromine. d. Bromin ...
... 1. a. Magnesium, chromium and sodium are all metals, hence, they react with oxygen to form basic oxides b. Chromium, as it is a transition metal. Metals have high density and coloured compounds are formed by transition metals. c. Bromine - the formula is Br2, that is, two atoms of bromine. d. Bromin ...
C1a - Mr Corfe
... to the left of the periodic table or further down in the group (not including groups 3-8) TYPES OF REACTIONS PHYSICAL – changing of states EXOTHERMIC – gives out heat ENDOTHERMIC – take in heat from it surrounding THERMAL DECOMPOSITION – is a chemical reaction where a single compound breaks up into ...
... to the left of the periodic table or further down in the group (not including groups 3-8) TYPES OF REACTIONS PHYSICAL – changing of states EXOTHERMIC – gives out heat ENDOTHERMIC – take in heat from it surrounding THERMAL DECOMPOSITION – is a chemical reaction where a single compound breaks up into ...
Name________________ Hour____ Chapter 11 Review 1. Name
... j. How many total atoms are reacting? 6 d. Name the element in the reaction. Oxygen k. How many total atoms are produced? 6 e. Name the compound on the reactant side. Carbon monoxide l. Which substances have double/triple g. List all of the subscripts in the reaction 2,2 bonds? All have double/tripl ...
... j. How many total atoms are reacting? 6 d. Name the element in the reaction. Oxygen k. How many total atoms are produced? 6 e. Name the compound on the reactant side. Carbon monoxide l. Which substances have double/triple g. List all of the subscripts in the reaction 2,2 bonds? All have double/tripl ...
C3 The Periodic Table
... • The old periodic table was rubbish – it was poorly ordered (based on patterns of behaviour, then on mass) and made little sense. • In 1964 Newlands attempted to put it in a sensible order by mass and saw similarities between every 8th ...
... • The old periodic table was rubbish – it was poorly ordered (based on patterns of behaviour, then on mass) and made little sense. • In 1964 Newlands attempted to put it in a sensible order by mass and saw similarities between every 8th ...
Halogens - Cronodon
... In elemental form, the halogens exist as simple molecular compounds, containing diatomic molecules (i.e. molecules of two atoms): F2, Cl2, Br2, I2. Fluorine is a paleyellow gas of F2 molecules, chlorine is a greenish-yellow gas of Cl2 molecules. Bromine is a reddish-orange liquid of Br2 molecules wi ...
... In elemental form, the halogens exist as simple molecular compounds, containing diatomic molecules (i.e. molecules of two atoms): F2, Cl2, Br2, I2. Fluorine is a paleyellow gas of F2 molecules, chlorine is a greenish-yellow gas of Cl2 molecules. Bromine is a reddish-orange liquid of Br2 molecules wi ...
Bromine
Bromine (from Greek: βρῶμος, brómos, meaning ""strong-smelling"" or ""stench"") is a chemical element with symbol Br, and atomic number 35. It is a halogen. The element was isolated independently by two chemists, Carl Jacob Löwig and Antoine Jerome Balard, in 1825–1826. Elemental bromine is a fuming red-brown liquid at room temperature, corrosive and toxic, with properties between those of chlorine and iodine. Free bromine does not occur in nature, but occurs as colorless soluble crystalline mineral halide salts, analogous to table salt.Bromine is rarer than about three-quarters of elements in the Earth's crust. The high solubility of bromide ions has caused its accumulation in the oceans, and commercially the element is easily extracted from brine pools, mostly in the United States, Israel and China. About 556,000 tonnes were produced in 2007, an amount similar to the far more abundant element magnesium.At high temperatures, organobromine compounds readily convert to free bromine atoms, a process which has the effect of stopping free radical chemical chain reactions. This effect makes organobromine compounds useful as fire retardants; more than half the bromine produced industrially worldwide each year is put to this use. Unfortunately, the same property causes sunlight to convert volatile organobromine compounds to free bromine atoms in the atmosphere, and an unwanted side effect of this process is ozone depletion. As a result, many organobromide compounds that were formerly in common use—such as the pesticide, methyl bromide—have been abandoned. Bromine compounds are still used for purposes such as in well drilling fluids, in photographic film, and as an intermediate in the manufacture of organic chemicals.Bromine has been long believed to have no essential function in mammals, but recent research suggests that bromine is necessary for tissue development. In addition, bromine is used preferentially over chlorine by one antiparasitic enzyme in the human immune system. Organobromides are needed and produced enzymatically from bromide by some lower life forms in the sea, particularly algae, and the ash of seaweed was one source of bromine's discovery. As a pharmaceutical, the simple bromide ion, Br−, has inhibitory effects on the central nervous system, and bromide salts were once a major medical sedative, before being replaced by shorter-acting drugs. They retain niche uses as antiepileptics.