Valence Electrons and Ionic Compounds · 价电子与离子化合物
| English | 中文 | Pinyin · 拼音 |
|---|---|---|
| valence electrons/ˈveɪləns ɪˈlektrɒnz/ | 价电子 | jià diàn zi |
| cations/ˈkætaɪənz/ | 阳离子 | yáng lí zi |
| anions/ˈænaɪənz/ | 阴离子 | yīn lí zi |
| ionic compound/aɪˈɒnɪk ˈkɒmpaʊnd/ | 离子化合物 | lí zi huà hé wù |
The outermost few
- An atom's chemistry is decided by just its outer few partners.
- The deep inner ones barely take part.
- Atoms swap or share these outer partners to become stable.
- Count them, and you can predict what an atom will do.
最外层的那几个
- 原子的化学性质只由它外层的那几个伙伴决定。
- 深处的内层几乎不参与。
- 原子交换或共享这些外层伙伴,以变得稳定。
- 数一数它们,你就能预测原子会做什么。
Valence electrons
- Valence electrons 价电子 are the outermost electrons.
- They decide how an atom bonds and reacts.
- A full outer shell -- an octet of 8 -- is especially stable.
价电子
- 价电子是最外层的电子。
- 它们决定原子如何成键和反应。
- 填满的外层——8 个电子的八隅体——特别稳定。
Valence electrons are the electrons in the... · 价电子位于……中
Valence electrons are the outermost ones and drive bonding. · 价电子是最外层的电子，驱动化学键的形成。
Atoms tend to gain or lose electrons to reach a full outer shell (an octet). · 原子倾向于获得或失去电子以达到满壳层（八隅体）。
A full octet is a low-energy, stable arrangement. · 完整的八隅体是一种低能量、稳定的结构。
Gaining and losing to become stable
- Metals lose valence electrons to form positive cations 阳离子.
- Nonmetals gain electrons to form negative anions 阴离子.
- Each aims for a full, noble-gas outer shell.
得失电子以变稳定
- 金属失去价电子,形成带正电的阳离子。
- 非金属得到电子,形成带负电的阴离子。
- 每个都力求达到填满的、稀有气体式的外层。
A metal atom that loses electrons becomes a... · 失去电子的金属原子变成……
Losing negative electrons leaves a net positive charge -- a cation. · 失去带负电的电子后留下净正电荷 —— 即阳离子。
Match each ion to its type. · 将每种离子与其类型匹配。
A plus sign marks a cation; a minus sign marks an anion. · 正号标记阳离子；负号标记阴离子。
Balancing the charges
- An ionic compound 离子化合物 is neutral overall.
- Combine cations and anions so the charges cancel.
- $\text{Na}^+$ with $\text{Cl}^-$ gives $\text{NaCl}$; $\text{Mg}^{2+}$ with $\text{Cl}^-$ gives $\text{MgCl}_2$.
平衡电荷
- 离子化合物整体上是中性的。
- 把阳离子和阴离子组合,使电荷相互抵消。
- $\text{Na}^+$ 与 $\text{Cl}^-$ 得 $\text{NaCl}$;$\text{Mg}^{2+}$ 与 $\text{Cl}^-$ 得 $\text{MgCl}_2$。
Form an ionic compound · 形成离子化合物
Transfer the metal's valence electron to the non-metal, making a cation and an anion. · 将金属的价电子转移到非金属上，形成阳离子和阴离子。
What is the neutral formula from $\text{Mg}^{2+}$ and $\text{Cl}^-$? · 由$\text{Mg}^{2+}$和$\text{Cl}^-$组成的中性化学式是什么？
One $2+$ needs two $1-$ ions to balance, giving $\text{MgCl}_2$. · 一个$2+$需要两个$1-$离子来平衡，从而形成$\text{MgCl}_2$。
How many $\text{Cl}^-$ ions balance one $\text{Al}^{3+}$ ion? · 多少个$\text{Cl}^-$离子能平衡一个$\text{Al}^{3+}$离子？
Three $1-$ ions cancel one $3+$, giving $\text{AlCl}_3$. · 三个$1-$离子抵消一个$3+$，得到$\text{AlCl}_3$。
Write the formula from magnesium ($\text{Mg}^{2+}$) and oxide ($\text{O}^{2-}$).
- The $2+$ and $2-$ cancel one-to-one.
- The formula is $\text{MgO}$.
用镁($\text{Mg}^{2+}$)和氧离子($\text{O}^{2-}$)写出化学式。
- $2+$ 和 $2-$ 一对一抵消。
- 化学式是 $\text{MgO}$。
Count only the outer-shell electrons as valence -- inner core electrons do not bond. Metals form cations (lose electrons), nonmetals form anions (gain electrons); do not mix these up. And an ionic formula must be electrically neutral, so choose subscripts that make the total positive charge equal the total negative (criss-cross the charges).
只把外层电子算作价电子——内层芯电子不成键。金属形成阳离子(失电子),非金属形成阴离子(得电子);别弄混。而且离子化学式必须是电中性的,所以要选择下标,使总正电荷等于总负电荷(把电荷交叉)。
Valence electrons are the outermost electrons that drive bonding, and atoms gain or lose them to reach a stable octet. Metals form cations and nonmetals form anions. An ionic compound balances these charges to stay neutral, so $\text{Mg}^{2+}$ and $\text{Cl}^-$ combine as $\text{MgCl}_2$.
价电子是驱动成键的最外层电子,原子通过得失它们来达到稳定的八隅体。金属形成阳离子,非金属形成阴离子。离子化合物平衡这些电荷以保持中性,所以 $\text{Mg}^{2+}$ 和 $\text{Cl}^-$ 组合成 $\text{MgCl}_2$。