Standard electrode potentials · 标准电极电位
| English | 中文 | Pinyin · 拼音 |
|---|---|---|
| electrode potential/ɪˈlektrəʊd pəˈtenʃl/ | 电极电势 | diàn jí diàn shì |
| half-cell/hɑːf sel/ | 半电池 | bàn diàn chí |
| cell potential/sel pəˈtenʃl/ | 电池电势 | diàn chí diàn shì |
| standard hydrogen electrode/ˈstændəd ˈhaɪdrədʒn ɪˈlektrəʊd/ | 标准氢电极 | biāo zhǔn qīng diàn jí |
| oxidising agent/ˈɒksɪdaɪzɪŋ ˈeɪdʒənt/ | 氧化剂 | yǎng huà jì |
| reducing agent/rɪˈdjuːsɪŋ ˈeɪdʒənt/ | 还原剂 | huán yuán jì |
Ranking the electron-grabbers
- The electrode potential 电极电势 $E$ shows how easily a half-cell 半电池 is reduced.
- We measure it against a fixed reference under standard conditions.
- Combining two half-cells gives a cell potential 电池电势.
给抢电子者排名
- 电极电位(electrode potential)$E$ 显示一个半电池有多容易被还原。
- 我们在标准条件下对一个固定的参考测量它。
- 结合两个半电池给出一个电池电位(cell potential)。
Electrode potential lab · 电极电位实验室
Ecell = Eright - Eleft
Change cell potential and see oxidising power increase. · 改变电池电位,看氧化能力增加。
A more negative standard electrode potential means a stronger reducing agent. · 一个更负的标准电极电位意味着一个更强的还原剂。
It loses electrons more readily. · 它更容易失去电子。
The reference and measuring E°
- The standard hydrogen electrode 标准氢电极 is the zero reference: $\text{H}_2$ at 1 atm over platinum in $1\ \dfrac{\text{mol}}{\text{dm}^3}$ $\text{H}^+$, defined as 0.00 V.
- To measure a half-cell's $E^{\ominus}$, connect it to the hydrogen electrode and read the voltage (always written as a reduction).
The electrochemical series of standard electrode potentials
参考和测量 E°
- 标准氢电极(standard hydrogen electrode)是零参考:$\text{H}_2$ 在 1 atm 通过铂在 $1\ \dfrac{\text{mol}}{\text{dm}^3}$ $\text{H}^+$ 中,定义为 0.00 V。
- 要测量一个半电池的 $E^{\ominus}$,把它连到氢电极并读电压(总是写成一个还原)。
标准电极电位的电化学序
The standard hydrogen electrode is defined as having a potential of: · 标准氢电极被定义为有以下哪个电位:
It is the reference half-cell, set at exactly 0.00 V; all other E° values are measured against it. · 它是参考半电池,设在恰好 0.00 V;所有其他 E° 值都对它测量。
Match each electrode-potential idea. · 匹配每个电极电位概念。
Each item links the term to its correct meaning. · 每一项把术语链接到它正确的含义。
Combining half-cells
- Polarity: the more negative electrode is the negative terminal; electrons flow from it through the circuit.
- Reactivity: a more positive $E^{\ominus}$ → better oxidising agent 氧化剂; a more negative $E^{\ominus}$ → better reducing agent 还原剂.
Electrolysis electroplates an object with a thin, shiny layer of metal such as chromium.
结合半电池
- 极性:更负的电极是负端;电子从它通过电路流动。
- 反应性:更正的 $E^{\ominus}$ → 更好的氧化剂;更负的 $E^{\ominus}$ → 更好的还原剂。
电解给一个物体电镀一层薄的、有光泽的金属如铬。
The standard cell potential is: · 标准电池电位是:
Subtract the less positive electrode potential from the more positive one. · 从更正的电极电位减去较不正的。
A half-cell with a more positive E° is: · 一个有更正 E° 的半电池是:
A more positive E° means the species is readily reduced — a stronger oxidising agent. · 一个更正的 E° 意味着该物种容易被还原——一个更强的氧化剂。
In a cell, electrons flow through the external circuit from the: · 在一个电池中,电子通过外电路从以下哪个流动:
The more negative electrode is the negative terminal; electrons flow from it to the more positive electrode. · 更负的电极是负端;电子从它流到更正的电极。
Reading the electrode-potential table
- The more positive E°, the more easily the species is reduced (a stronger oxidising agent).
- The more negative, the stronger the reducing agent.
The standard hydrogen electrode reference
读取电极电位表
- E° 越正,该物种越容易被还原(一个更强的氧化剂)。
- 越负,还原剂越强。
标准氢电极参考
You've got it
- $E^{\ominus}$ shows how easily a half-cell is reduced (written as a reduction)
- the standard hydrogen electrode = 0.00 V reference
- $E^{\ominus}_{\text{cell}} = E^{\ominus}(\text{more positive}) - E^{\ominus}(\text{less positive})$
- more positive $E^{\ominus}$ = stronger oxidising agent; more negative = stronger reducing agent
你掌握了
- $E^{\ominus}$ 显示一个半电池有多容易被还原(写成一个还原)
- 标准氢电极 = 0.00 V 参考
- $E^{\ominus}_{\text{cell}} = E^{\ominus}(\text{more positive}) - E^{\ominus}(\text{less positive})$
- 更正的 $E^{\ominus}$ = 更强的氧化剂;更负的 = 更强的还原剂