Unit 2: Atoms and Ions Homework Booklet
... c. When coal is burned a gas is given off that is weakly soluble in water. What is the gas and what is formed when it dissolves in water? ...
... c. When coal is burned a gas is given off that is weakly soluble in water. What is the gas and what is formed when it dissolves in water? ...
First, there are several issues regarding this course need to be
... In order to apply the Born equation (10.2), we need to know the radius of the corresponding ions. These numbers can be obtained from Table 23.3 r(Br-) = 196 pm; r(Cl-) = 181 pm; thus ∆solvGө(Br-, aq) - ∆solvGө (Cl-, aq) = - (1/196 – 1/181)*6.86*104 kJ mol-1 = 29.00 kJ mol-1 (The calculated result is ...
... In order to apply the Born equation (10.2), we need to know the radius of the corresponding ions. These numbers can be obtained from Table 23.3 r(Br-) = 196 pm; r(Cl-) = 181 pm; thus ∆solvGө(Br-, aq) - ∆solvGө (Cl-, aq) = - (1/196 – 1/181)*6.86*104 kJ mol-1 = 29.00 kJ mol-1 (The calculated result is ...
Physics and Chemistry 3º ESO Techniques to separate the
... 3. Remove the thermometer and place a boiling chip and about 75ml of wine using a long-stem funnel into the distilling flask. 4. Turn on the cooling water and have the instructor check your setup, then apply the heat to the wine. After boiling begins, reduce the heat so the wine boils at a moderate ...
... 3. Remove the thermometer and place a boiling chip and about 75ml of wine using a long-stem funnel into the distilling flask. 4. Turn on the cooling water and have the instructor check your setup, then apply the heat to the wine. After boiling begins, reduce the heat so the wine boils at a moderate ...
C:\usb key\sch3u\unit 1\chapter 2 test answers.wpd
... London forces; dipole/dipole forces; Hydrogen bonds; Covalent and Ionic 11) Which compound in each of the following pairs of compounds will have the higher melting point? Give the deciding factor in each case. a) NH3 and PH3 b) LiBr and SBr2 c) BCl3 and BCl2F d) C4H10 and C12H26 ...
... London forces; dipole/dipole forces; Hydrogen bonds; Covalent and Ionic 11) Which compound in each of the following pairs of compounds will have the higher melting point? Give the deciding factor in each case. a) NH3 and PH3 b) LiBr and SBr2 c) BCl3 and BCl2F d) C4H10 and C12H26 ...
SCIENCE 10: Chemical Reactions – Atomic Structure
... The element copper forms two different compounds with chlorine. Chlorine always forms a 1- ion. Copper can form either a 1+ ion or a 2+ ion. CuCl = copper (I) chloride CuCl2 = copper (II) chloride Naming Ionic Compounds: (p.194) o Metal name first, non-metal name second o Change the ending of the ...
... The element copper forms two different compounds with chlorine. Chlorine always forms a 1- ion. Copper can form either a 1+ ion or a 2+ ion. CuCl = copper (I) chloride CuCl2 = copper (II) chloride Naming Ionic Compounds: (p.194) o Metal name first, non-metal name second o Change the ending of the ...
North Haven Public Schools Curriculum
... The atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form. Lewis dot structures can provide models of atoms and molecules. The shape of simple molecules and their polarity ca ...
... The atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form. Lewis dot structures can provide models of atoms and molecules. The shape of simple molecules and their polarity ca ...
Matter and Measurement
... Example: Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of calcium chloride and sodium carbonate are mixed. First write the chemical formulas of the reactants aqueous Calcium chloride: CaCl2(aq) aqueous sodium carbonate: Na2CO3(aq) Next, determine wha ...
... Example: Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of calcium chloride and sodium carbonate are mixed. First write the chemical formulas of the reactants aqueous Calcium chloride: CaCl2(aq) aqueous sodium carbonate: Na2CO3(aq) Next, determine wha ...
Chapter 7 Ionic and Metallic Bonding
... The Electron Dot diagram for Nitrogen Nitrogen has 5 valence electrons to show. First we write the symbol. Then add 1 electron at a time to each side. Now they are forced to pair up. We have now written the electron dot diagram for Nitrogen. ...
... The Electron Dot diagram for Nitrogen Nitrogen has 5 valence electrons to show. First we write the symbol. Then add 1 electron at a time to each side. Now they are forced to pair up. We have now written the electron dot diagram for Nitrogen. ...
Solutions
... have higher boiling points than pure solvents. This is true with solid solutes and heavier liquid solutes. Other liquid solutes may form azeotropes, which are mixtures with lower boiling points than either solute or solvent – example 95% ethanol/water.) Solutes raise the boiling point of liquids ...
... have higher boiling points than pure solvents. This is true with solid solutes and heavier liquid solutes. Other liquid solutes may form azeotropes, which are mixtures with lower boiling points than either solute or solvent – example 95% ethanol/water.) Solutes raise the boiling point of liquids ...
Alkali Metals They are very similar in properties than any other
... o Halogens can combine with each other to form interhalogens and polyhalide. o Polyhalide ions have the general formula [Y-X-Y]. Not possible for F to represent X in a polyhalide as it cannot expand its octet. Hydrides: o Hydrogen halides formula – HX. HF is a colorless liquid which boils at 19. ...
... o Halogens can combine with each other to form interhalogens and polyhalide. o Polyhalide ions have the general formula [Y-X-Y]. Not possible for F to represent X in a polyhalide as it cannot expand its octet. Hydrides: o Hydrogen halides formula – HX. HF is a colorless liquid which boils at 19. ...
Exercised Review for Test
... 4. A molecule in which one end is slightly negative and the other end is slightly positive ...
... 4. A molecule in which one end is slightly negative and the other end is slightly positive ...
Unit 8-10 Review Answers
... (a) Molecules in a liquid are much more closely packed than molecules in a gas. (b) Molecules in a liquid can vibrate and rotate, but they cannot move about freely as molecules in a gas. (c) Liquids are much more difficult to compress into a smaller volume than are gases. (d) Liquids diffuse more sl ...
... (a) Molecules in a liquid are much more closely packed than molecules in a gas. (b) Molecules in a liquid can vibrate and rotate, but they cannot move about freely as molecules in a gas. (c) Liquids are much more difficult to compress into a smaller volume than are gases. (d) Liquids diffuse more sl ...
Phase-separation in ion-containing mixtures in electric fields
... separates into its components when put under the In the absence of field (mixed state) and under coninfluence of an electric field in some reasonable condi- stant applied external stress, the mixture will have tions. The dissociated ions in the solution are impor- the homogeneous viscosity ηm , and ...
... separates into its components when put under the In the absence of field (mixed state) and under coninfluence of an electric field in some reasonable condi- stant applied external stress, the mixture will have tions. The dissociated ions in the solution are impor- the homogeneous viscosity ηm , and ...
Critical Assessment of the Formation of Ionic-Liquid - PATh
... acids,27 more hydrophobic, yet water-soluble ionic liquids must be employed. Such ionic liquids are here defined as those fluids composed of long alkyl side chain lengths and/or anions with low hydrogen bond basicity values,8,11 namely [N(CN)2], [CF3SO3], and [BF4]. Although it was previously21 sho ...
... acids,27 more hydrophobic, yet water-soluble ionic liquids must be employed. Such ionic liquids are here defined as those fluids composed of long alkyl side chain lengths and/or anions with low hydrogen bond basicity values,8,11 namely [N(CN)2], [CF3SO3], and [BF4]. Although it was previously21 sho ...
Net ionic equation
... Reactions of acids and bases •Neutralization: acid + base are mixed: HNO3(aq) + KOH(aq) ??? •Salt = ionic compound cation from base anion from acid. •Neutralization of acid with metal hydroxide produces water and a salt. •Acids + carbonates = CO2 and H2O ...
... Reactions of acids and bases •Neutralization: acid + base are mixed: HNO3(aq) + KOH(aq) ??? •Salt = ionic compound cation from base anion from acid. •Neutralization of acid with metal hydroxide produces water and a salt. •Acids + carbonates = CO2 and H2O ...
Dangerous Goods - `OnGuard®` Safety Training
... prevent contact with in flowing liquids such as rain. Appropriate spillage clean-up and personal protective equipment should be provided and kept in good order. The type of clean-up and personal protective equipment required, willdepend on the quantities of DG, their types and handling methods. The ...
... prevent contact with in flowing liquids such as rain. Appropriate spillage clean-up and personal protective equipment should be provided and kept in good order. The type of clean-up and personal protective equipment required, willdepend on the quantities of DG, their types and handling methods. The ...
AP Chemistry Unit 1 Essential Questions Screencast 1
... Screencast 1-1 Introduction to the Periodic Table 1. What is an element? 2. How are the symbols for the elements determined? 3. How is the order of the elements determined on the modern periodic table? 4. What are the main regions of the periodic table? 5. What are the special named groups and where ...
... Screencast 1-1 Introduction to the Periodic Table 1. What is an element? 2. How are the symbols for the elements determined? 3. How is the order of the elements determined on the modern periodic table? 4. What are the main regions of the periodic table? 5. What are the special named groups and where ...
Atomic arrangement, short and long range order, point. Direction
... which means that long-range order does not exist in liquids and amorphous solids. In crystals, the atoms are arranged in regular rows or networks (in threedimensional lattices), and aregular alternation of atoms separated by the same distances is repeated for atoms separated byany distance—that is, ...
... which means that long-range order does not exist in liquids and amorphous solids. In crystals, the atoms are arranged in regular rows or networks (in threedimensional lattices), and aregular alternation of atoms separated by the same distances is repeated for atoms separated byany distance—that is, ...
Lecture 35 (Slides) November 7
... • The normal boiling point of water is 100 oC. At this temperature the vapor pressure of water is exactly 760mm Hg (the normal average atmospheric pressure at sea level). If we heat water in a sealed container all of the steam that is formed is trapped above the liquid water. The additional steam fo ...
... • The normal boiling point of water is 100 oC. At this temperature the vapor pressure of water is exactly 760mm Hg (the normal average atmospheric pressure at sea level). If we heat water in a sealed container all of the steam that is formed is trapped above the liquid water. The additional steam fo ...
Bonding - Graham ISD
... is the noble gases (group 18). This is true because compounds of these atoms are almost always less stable than the original atom. Atoms with a partially stable outer energy level can lose, gain, or share electrons to obtain a stable outer energy level. ...
... is the noble gases (group 18). This is true because compounds of these atoms are almost always less stable than the original atom. Atoms with a partially stable outer energy level can lose, gain, or share electrons to obtain a stable outer energy level. ...
Chapter 7 Ionic and Metallic Bonding
... explain why atoms form certain kinds of ions and molecules The Octet Rule: in forming compounds, atoms tend to achieve a noble gas configuration; 8 in the outer level is stable Each noble gas (except He, which has 2) has 8 electrons in the outer level ...
... explain why atoms form certain kinds of ions and molecules The Octet Rule: in forming compounds, atoms tend to achieve a noble gas configuration; 8 in the outer level is stable Each noble gas (except He, which has 2) has 8 electrons in the outer level ...
Chapter 6 Chemical Bonding
... unequal attraction for the shared electrons Ex: H-F Polar molecules have an unbalanced distribution of electrons, thus have two regions of different electric charges Ex: Water Percentage of Ionic character of a bond A-B, X is electronegativity XA - XB % I.C. = ---------------------- * 100% XA Ex: Na ...
... unequal attraction for the shared electrons Ex: H-F Polar molecules have an unbalanced distribution of electrons, thus have two regions of different electric charges Ex: Water Percentage of Ionic character of a bond A-B, X is electronegativity XA - XB % I.C. = ---------------------- * 100% XA Ex: Na ...
Chapter 13
... number of particles in solution. This is most easily done by using the van 't Hoff factor i as mB = msolute · i. The factor i accounts for the number of individual particles (typically ions) formed by a compound in solution. ...
... number of particles in solution. This is most easily done by using the van 't Hoff factor i as mB = msolute · i. The factor i accounts for the number of individual particles (typically ions) formed by a compound in solution. ...
Ionic strength effect on the deprotonation of para
... Abstract: The deprotonation of para-sulfonatocalix[4]arene was studied by a combination of spectrophotometric and potentiometric methods at 25 °C. The ionic strength of the solutions was kept constant by sodium perchlorate as a background electrolyte at 0.10–4.0 mol dm-3. The spectral changes eviden ...
... Abstract: The deprotonation of para-sulfonatocalix[4]arene was studied by a combination of spectrophotometric and potentiometric methods at 25 °C. The ionic strength of the solutions was kept constant by sodium perchlorate as a background electrolyte at 0.10–4.0 mol dm-3. The spectral changes eviden ...
Chemical Formulas
... single atom Na+ or S2- usually tell by column on periodic table, some elements have more than one oxidation number or charge Binary compounds- only 2 elements in the compound Na2S Polyatomic ions - ions formed from more than one type of atom covalently bonded together OHPO43- NH4+ ...
... single atom Na+ or S2- usually tell by column on periodic table, some elements have more than one oxidation number or charge Binary compounds- only 2 elements in the compound Na2S Polyatomic ions - ions formed from more than one type of atom covalently bonded together OHPO43- NH4+ ...
Ionic liquid
An ionic liquid (IL) is a salt in the liquid state. In some contexts, the term has been restricted to salts whose melting point is below some arbitrary temperature, such as 100 °C (212 °F). While ordinary liquids such as water and gasoline are predominantly made of electrically neutral molecules, ionic liquids are largely made of ions and short-lived ion pairs. These substances are variously called liquid electrolytes, ionic melts, ionic fluids, fused salts, liquid salts, or ionic glasses. Ionic liquids have many applications, such as powerful solvents and electrically conducting fluids (electrolytes). Salts that are liquid at near-ambient temperature are important for electric battery applications, and have been used as sealants due to their very low vapor pressure.Any salt that melts without decomposing or vaporizing usually yields an ionic liquid. Sodium chloride (NaCl), for example, melts at 801 °C (1,474 °F) into a liquid that consists largely of sodium cations (Na+) and chloride anions (Cl−). Conversely, when an ionic liquid is cooled, it often forms an ionic solid—which may be either crystalline or glassy.The ionic bond is usually stronger than the Van der Waals forces between the molecules of ordinary liquids. For that reason, common salts tend to melt at higher temperatures than other solid molecules. Some salts are liquid at or below room temperature. Examples include compounds based on the 1-Ethyl-3-methylimidazolium (EMIM) cation and include: EMIM:Cl, EMIM dicyanamide, (C2H5)(CH3)C3H3N+2·N(CN)−2, that melts at −21 °C (−6 °F); and 1-butyl-3,5-dimethylpyridinium bromide which becomes a glass below −24 °C (−11 °F).Low-temperature ionic liquids can be compared to ionic solutions, liquids that contain both ions and neutral molecules, and in particular to the so-called deep eutectic solvents, mixtures of ionic and non-ionic solid substances which have much lower melting points than the pure compounds. Certain mixtures of nitrate salts can have melting points below 100 °C.The term ""ionic liquid"" in the general sense was used as early as 1943.