美国高中化学酸碱反应 Acid-Base Reactions
高中化学英文词汇
高中化学英文词汇High School Chemistry English VocabularyChemistry is a fascinating subject that explores the composition, properties, and behavior of matter. Whether you are a high school student diving into the world of chemistry for the first time or a seasoned science enthusiast, it is essential to have a good understanding of the English vocabulary commonly used in this field. In this article, we will introduce some key terms and concepts in high school chemistry, along with their English equivalents.1. Elements and AtomsIn chemistry, an element is a pure substance that cannot be broken down into simpler substances by chemical means. Each element is made up of atoms, which are the smallest units of matter that retain the properties of the element. Some common elements include hydrogen, oxygen, carbon, and nitrogen.2. Compounds and MoleculesCompounds are substances composed of two or more elements chemically combined in fixed proportions. The smallest unit of a compound is called a molecule, which consists of two or more atoms bonded together. Water (H2O) and carbon dioxide (CO2) are examples of compounds.3. Chemical ReactionsChemical reactions involve the breaking and forming of chemical bonds between atoms. During a chemical reaction, reactants are transformed intoproducts through the rearrangement of atoms. Some common types of chemical reactions include synthesis, decomposition, combustion, and single displacement.4. Acids and BasesAcids are substances that donate protons (H+) in a chemical reaction, while bases are substances that accept protons. The strength of an acid or base is determined by its pH level, with acids having a pH below 7 and bases having a pH above 7. Examples of acids include hydrochloric acid (HCl) and sulfuric acid (H2SO4), while common bases include sodium hydroxide (NaOH) and ammonia (NH3).5. Chemical EquationsChemical equations are symbolic representations of chemical reactions, with reactants on the left side and products on the right side. Coefficients are used to balance chemical equations and ensure the conservation of mass. For example, the reaction between hydrogen gas (H2) and oxygen gas (O2) to form water can be represented as 2H2 + O2 → 2H2O.6. States of MatterMatter can exist in three states: solid, liquid, and gas. Solids have a fixed shape and volume, liquids have a fixed volume but can change shape, and gases have neither a fixed shape nor volume. Changes in temperature and pressure can cause substances to change states, such as melting, freezing, boiling, and condensation.7. The Periodic TableThe periodic table is a tabular arrangement of the elements based on their atomic number and chemical properties. Elements are organized into groups and periods, with similar properties grouped together. The periodic table provides valuable information about the properties of elements, such as their atomic mass, symbol, and electron configuration.8. StoichiometryStoichiometry is the branch of chemistry that deals with the calculation of quantities of reactants and products in a chemical reaction. It involves balancing chemical equations, determining the limiting reactant, and calculating the theoretical yield of a reaction. Stoichiometry is essential for understanding the composition of compounds and predicting the outcome of reactions.In conclusion, mastering the English vocabulary of high school chemistry is crucial for success in the subject. By familiarizing yourself with key terms and concepts, you can enhance your understanding of chemical principles and communicate effectively with peers and educators. Remember to review and practice these terms regularly to solidify your knowledge and confidence in the exciting world of chemistry.。
美国高中化学酸碱反应 Acid-Base Reactions
• What types of acid-base reactions do these titration graphs show?
Titrations practice
Titrations practice
• Graphs shows titration of 0.5 M NaOH with 50ml of an unknown acid. After titration NaBr salt crystals were isolated from the solution. a) What is the acid used? Is it strong or e produced from an acid-base reaction
Regulating pH
• Living things interact with acids and bases all the time; their pH must be regulated • Buffer
• How do we know the Standard solution is neutral? • pH Indicators酸碱指示剂
• End point • Equivalence point • Neutral point
– Volume of acid/base used gives us molarity – MAVA = MBVB
Titrations practice
• If 15.0 mL of 0.50 M NaOH is used to neutralize 25.0 mL of HC2H3O2, what is the molarity of the acid solution? NaOH + HC2H3O2 H2O + NaC2H3O2; 1:1 ratio • MAVA = MBVB • MA= MBVB/VA = (0.50 M)(15.0 ml)/25.0 ml = 0.30 M • If 25.0 mL of a standard 0.05 M HCl solution is required to neutralize 20.0 mL of a solution of Sr(OH)2, what is the concentration of the base? 2 HCl + Sr(OH)2 SrCl2 + 2H2O; 2:1 ratio • MAVA = 2 MBVB • MB = MAVA/2VB = (0.05 M)(25.0 ml)/(2)(20.0 ml) = 0.03 M
SAT化学词汇
附录三名词总结第二章正电荷(positive charge)原子核(atomic nucleus)负电荷(negative charge)质子(proton)中子(neutron)道尔顿模型(Dalton Model)汤姆逊模型(Thomason Model)库伦(coulomb)卢瑟福模型(Rutherford Model)波尔模型(N.Bohr Model)原子轨道学说(Atomic Orbital Hypothesis) 基态(ground state)激发态(excited state)电离(ionization)普朗克常数(Planck’s constant)频率(frequency)波长(wavelength)物质波假设(The L.de Broglie Hypothesis) 电子衍射实验(electron diffraction experiment)海森堡测不准原则(Heisenberg Uncertainty Principle)位置(position)动量(momentum)量子数(quantum number)电子层(shells)亚层(subshells)轨道(orbit)主量子数(Principal Quantum Number)角量子数(Azimuthal Quantum Number)磁量子数(Magnetic Quantum Number)自旋量子数(Spin Quantum Number)电子排布(Electron Configuration)保利不相容原理(Pauli’s Exclusion Principle)能量最低原理(Lowest Energy Principle, Aufbau Principle) 价电子(valence electron)洪特规则(Hund's Rules)能级交错原理(energy overlay)元素周期表（the Periodic Table）原子序数(Atomic Number)同位素(Isotope)质量数(Mass Number)原子质量(Atomic Masses)周期(period)族(group)主族(main group)碱金属(alkali metal)碱土金属(alkaline earth metal)卤素(halogen)惰性气体(noble gas)硼族元素(boron group element)碳族元素(carbon group element)氮族元素(nitrogen group element)氧族元素(oxygen group element)。
酸碱理论
＿
4．用质子理论来解释一些反应：
(1) 气相中的酸碱反应： HCl(g)
A1
(2) 离解反应（dissociation reactions）：
H+
a. auto ionization ： H2O
+ H+
H2O
Kw
H3O
+
+
OH
＿
b. acid ionization ： HAc
− 、 HCO 3 ? What is the conjugate acid of each of the following bases： CN − 、 H 2S 、 PH + 4 − − 、 H 2 O 、 HCO 3 ? SO 2 4
－
H+ + NH3(g) B2
＋
Lewis base
－
acid−base adduct H2O
(1) adduct reaction：H + : OH
Cu 2 + + 4NH + 4 2+ (3) substitution reaction of base： Cu(NH 3 ) 4 + 2OH Cu(OH) 2 + 4NH 3 (4) both substitution reaction：Ba(OH)2 + H2SO4 BaSO4↓+2H2O 4．优点： (1) 它包括了水离子论、溶剂论、质子论三种理论； (2) 它扩大了酸的范围。 5．缺点：无统一的酸碱强度的标度。 由于电子论包括了所有的酸碱理论， 所以该理论又称为广义酸碱理论。 酸碱电子论的提 出，可以把所有的化学反应分为三大类：
酸碱滴定法acid-basetitration
① 强酸（碱）溶液
C mol/L HCl
[H+]=[OH-]+[Cl-]=
Kw [H
]
C HCl
CHCl > 10-6 mol/l → [H+] = CHCl
② 弱酸（碱）溶液
a. 一元弱酸（碱）
HA Ka H+ + A-
[H+][A-] Ka = [HA]
[H+]=[]+[A-]=
Kw [H
1. 指示剂+惰性染料（背景）
甲基橙色
PH≥4.4 黄 PH＝4.1 橙 PH≤3.1 红
甲基橙+靛蓝色
绿 浅灰 紫
2. 二种以上指示剂混合， 使变色点更符合计量点
溴甲酚绿-甲基红: PH<3.8: 黄 + 红→ 酒红（橙） PH＝5.1：接近无色 PH>6.2：蓝 + 黄→ 绿
酸碱溶液酸碱度的计算
TE% [OH- ]-[HA] -[H ] 100% Csp
由于强碱滴定弱酸化学计量点溶液呈碱性， 故[H+]可略去，又因为[HA]/CSP=δHA
上式可简化为：
TE%
[OH (
Csp
]
HA
)
100%
Csp=C0·V0/Vep, C0, V0为被测物质的原始浓度 和体积， Vep为计量点时溶液的体积。
酚酞：有机弱酸Pka=9.1
羟式
醌式
甲基橙：有机弱碱
偶氮式 醌式
现以HIn代表弱酸指示剂，其离解平衡表示如下：
HIn H+ + In酸式色 碱式色
以InOH代表弱碱指示剂，其离解平衡表示如下：
生物化学考研精解名词解释答案(上)版
生化考研精解名词解释答案（上）温馨提示：部分解释不是采自教材，如有疑问，请参考课本！第一章糖类（p6）6.构型（configuration）：在立体化学中，因分子中存在不对称中心而产生的异构体中的原子或取代基团的空间排列关系。
有D型和L型两种。
构型的改变要有共价键的断裂和重新组成，从而导致光学活性的变化。
7.构象（conformation）：分子中由于共价单键的旋转所表现出的原子或基团的不同空间排列。
指一组结构而不是指单个可分离的立体化学形式。
构象的改变不涉及共价键的断裂和重新组成，也无光学活性的变化。
12.差向异构体（epimer）：在立体化学中，含有多个手性碳原子的立体异构体中，只有一个手性碳原子的构型不同，其余的构型都相同的非对映体叫差向异构体。
14.异头碳（anomeric carbon）：单糖由直链变成环状结构时，羰基碳原子成为新的手性中心，导致C1差向异构化，产生两个非对映异构体。
在环状结构中，半缩醛碳原子称为异头碳原子。
15.半缩醛（hemiacetal）：醛基和一个醇基缩合形成的产物。
通过该反应，使单糖形成环状结构。
16.变旋（mutarotation）：当一种旋光异构体如糖，溶于水中转变成几种不同旋光异构体的平衡混合物时，随着时间而发生的旋光变化。
18.糖苷键（glycosidic bond）：一个单糖或糖链还原端半缩醛上的羟基与另一个分子(如醇、糖、嘌呤或嘧啶)的羟基、胺基或巯基之间缩合形成的缩醛键或缩酮键。
常见的糖苷键有O-糖苷键和N-糖苷键。
19.还原糖（reducing sugar）：能够还原斐林(H.von Fehling)试剂或托伦斯(B.Tollens)试剂的糖称为还原糖，所有的单糖（除二羟丙酮），不论醛糖、酮糖都是还原糖。
大部分双糖也是还原糖，蔗糖例外。
22.淀粉（starch）：由D-葡萄糖单体组成的同聚物。
包括直链淀粉和支链淀粉两种类型，为植物中糖类的主要贮存形式。
Lewis酸碱理论
Lewis酸碱理论理论发展布朗斯特酸碱理论概念的核心系于分子或离子间的质子转移，显然无法对不涉及质子转移，但却具有酸碱特征的反应做解释.这一不足在布朗斯特概念提出的同年由美国化学家路易斯提出的酸碱电子理论（the electronic theory of acid and alkali），也称广义酸碱理论、路易斯（lewis）酸碱理论，是1923年美国物理化学家吉尔伯特·牛顿·路易斯（Lewis G N）提出的一种酸碱理论，它认为：凡是可以接受外来电子对的分子、基团或离子为酸；凡可以提供电子对的分子、离子或原子团为碱。
这种理论包含的酸碱范围很广，但是，它对确定酸碱的相对强弱来说，没有统一的标度，对酸碱的反应方向难以判断。
后来，皮尔逊提出的软硬酸碱理论弥补了这种理论的缺陷。
电子酸碱该理论认为：凡是能够接受外来电子对的分子、离子或原子团称为路易斯酸（Lewis acid)，即电子对接受体，简称受体；凡是能够给出电子对的分子、离子或原子团称为路易斯碱（Lewis base），即电子对给予体，简称给体。
或者说：路易斯酸（Lewis acid)是指能作为电子对接受体（Electron pair acceptor）的原子，分子，离子或原子团；路易斯碱（Lewis base)则指能作为电子对给予体（Electron pair donor）的原子，分子，离子或原子团；酸碱反应是电子对接受体与电子对给予体之间形成配位共价键的反应.路易斯酸的分类1、配位化合物中的金属阳离子，例如[Fe(H2O)6]3+和[Cu(NH3）4]2+中的Fe3+离子和Cu2+离子.2、有些分子和离子的中心原子尽管满足了8电子结构，仍可扩大其配位层以接纳更多的电子对.如 SiF4 是个路易斯酸，可结合2个F–的电子对形成[SiF6]2–.3、另一些分子和离子的中心原子也满足8电子结构，但可通过价层电子重排接纳更多的电子对.再如CO2能接受OH–离子中O 原子上的孤对电子4、某些闭合壳层分子可通过其反键分子轨道容纳外来电子对.碘的丙酮溶液呈现特有的棕色，是因为I2分子反键轨道接纳丙酮中氧原子的孤对电子形成配合物（CH3）2COI2.再如四氰基乙烯（TCNE）的π*轨道能接受一对孤对电子。
分析化学英文课件04 酸碱平衡Acid-Base Equilibria
Autoprotolysis
As the elemental unit of positive charge, the proton possesses a charge density which makes its independent existence in a solution extremely unlikely. Thus, in order to transform HB into B-, a proton acceptor must be present. Often as in the dissociation of acetic acid in water, this base may be the solvent(H2O) itself.
HAc = H+ + Ac- , H2O + H+ = H3O+
Combination of this two equations, HAc + H2O = H3O+ + Ac-
The protonated water molecule or hydrated proton H3O+, may be called a “hydronium ion”, but it is usually designated simply by “hydrogen ion” and often written as “H+”.
According to Arrhenius theory, acids dissociate into
hydrogen ions and anions, and bases dissociate into
hydroxide ions and cations.
- 1、下载文档前请自行甄别文档内容的完整性，平台不提供额外的编辑、内容补充、找答案等附加服务。
- 2、"仅部分预览"的文档,不可在线预览部分如存在完整性等问题,可反馈申请退款(可完整预览的文档不适用该条件!)。
- 3、如文档侵犯您的权益，请联系客服反馈,我们会尽快为您处理(人工客服工作时间：9:00-18:30)。
Weak Acid + Strong Base
• HC2H3O2(aq) + NaOH(aq) • Weak acid wont completely dissociate
– Wont breakdown into ions on reaction side HC2H3O2(aq) + Na+(aq)+OH-(aq)Na+(aq)+C2H3O2-(aq)+ H2O(l)
H+(aq)+Cl-(aq)+Al(OH)3(s)Al+3(aq)+Cl-(aq)+H2O(l) H+(aq)+Al(OH)3(s)Al+3(aq)+H2O(l) • End solution is slightly acidic • What about NH3?
– Considered a weak base but has no OH– Does not produce water H+(aq)+Cl-(aq)+NH3(aq)NH4++Cl-(aq) H+(aq))+NH3(aq)NH4+ – HCl(aq)+NH3(aq)NH4Cl(aq)
Strong Acid + Strong Base
• HCl + NaOH NaCl + HOH • Double replacement reaction • Both compounds completely dissociate
HCl Cl- + H+ NaOH Na+ + OH-
• Complete equation (aq) can be written: H++Cl-+Na++OH-Cl-+Na++H2O • Spectator Ions
Strong Acid + Strong Base
• What is the net ionic equation: HCl(aq) + NaOH(aq) 1) H+(aq) +Cl-(aq) +Na+(aq) +OH-(aq) Cl-(aq) +Na+(aq) +H2O(aq) 2) H+(aq) +OH-(aq) H2O(l) • All strong acid and strong base reactions have this as a base net ionic equation KOH(aq)+HNO3(aq)KNO3(aq)+H2O(l) K++OH-+H++NO3- K++NO3-+H2O(l) OH-+H++ H2O(l)
– H2CO3 increases making blood more acidic
• What kind of blood pH results in yawning?
– Acidic blood; body needs to release large amount of CO2 by taking in large amount of O2
• HCl(aq) + Al(OH)3(s) • Weak bases wont completely dissociate
Strong Acid + Weak Base
– Cannot write them as ions on reaction side of net ionic equation
Bronsted-Lowery Acids and Bases
H2O(l)+NH3(aq)NH4+(aq)+OH-(aq)
ACID BASE Conjugate acid Conjugate base
• • • •
Acid= Any compound that releases H+ Base= Any compound that takes H+ Water can act as an acid or a base Conjugate Acid/Base
Acid-Base Reactions Ch. 15
• Neutralization reactions中和反应
– pH is changed
Acid-Base Reactions
• Produce a salt and H2O
• 2 types of Acids
– Strong and Weak
HC2H3O2(aq) +OH-(aq)C2H3O2-(aq)+ H2O(l) • End solution is slightly basic Weak Acid + Weak Base ???Not clear??? • Both the acid and base are so unreactive there is little change • Not common reaction type in nature
Add a strong base: HC2H3O2(aq)+NaOH(aq) C2H3O2-(aq)+H2O(l) HC2H3O2(aq)+OH-(aq) C2H3O2-(aq)+H2O(l)
• Weak acid/base + salt of that acid/base NaC2H3O2 and HC2H3O2
– Solution that adjusts to the addition of acids and bases to slowly change the pH Add a strong acid: - and H+ ions – Free OH NaC2H3O2(aq)+HCl(aq)
HC2H3O2(aq)+NaCl(l) C2H3O2-(aq)+H+(aq)HC2H3O2(aq)
HBr: NaOH + HBr NaBr + H2O; strong
b) what is the concentration of the acid used?
MA= MBVB/VA = (0.5M)(35ml)/50ml = 0.35 M
• What types of acid-base reactions do these titration graphs show?
Titrations practice
Titrations practice
• Graphs shows titration of 0.5 M NaOH with 50ml of an unknown acid. After titration NaBr salt crystals were isolated from the solution. a) What is the acid used? Is it strong or weak?
NaOH + HC2H3O2H2O + NaC2H3O2
Buffers in the Blood
• Blood must keep a pH of 7.4 to allow the best exchange of CO2 and O2 • Blood buffer is HCO3-/H2CO3 • Add Base: H2CO3+OH-HCO3-+H2O • Add Acid: HCO3-+H+H2CO3 • What happens when you take in too much CO2?
– Ions that do not take part in the reaction
Net Ionic Equations净离子方程式
1) Write Complete Ionic Equation
All soluble compounds are shown as free ions
2) Remove Spectator Ions Ions not directly evolved in the rxn. 3) Balance the remaining rxn.
• How do we know the Standard solution is neutral? • pH Indicators酸碱指示剂
• End point • Equivalence point • Neutral point
– Volume of acid/base used gives us molarity – MAVA = MBVB
H2O
• Test to determine the molarity of an acid or a base • Process:
Titrations滴定
– Find the Standard Solution标准溶液 – Standard solution of an acid/base is slowly added to an acid/base of unknown molarity – When the unknown acid/base is neutral, the [H+]=[OH-]
– Salts are ionic compounds
• 2 types of Bases
– Strong and Weak
• 4 possible combinations of Acids and Bases
– – – – Strong A + Strong B Strong A + Weak B Weak B + Strong B Weak B + Weak A