高中化学方程式总结大全 一、非金属单质(F 2 ,Cl 2 ,O 2 ,S,N 2 ,P,C,Si,H) 1、氧化性: F 2 +H 2 ===2HF (阴暗处爆炸) F 2 +Xe (过量) ==XeF 2 2F 2 (过量) +Xe==XeF 4 (XeF 4 是强氧化剂,能将 Mn 2+ 氧化为 MnO 4– ) nF 2 +2M===2MFn(M 表示大部分金属) 2F 2 +2H 2 O===4HF+O 2 (水是还原剂) 2F 2 +2NaOH===2NaF+OF 2 +H 2 O F 2 +2NaCl===2NaF+Cl 2 F 2 +2NaBr===2NaF+Br 2 F 2 +2NaI===2NaF+I 2 7F 2 (过量) +I 2 ===2IF 7 F 2 +Cl 2 (等体积) ===2ClF (ClF 属于类卤素:ClF+H 2 O==HF+HClO ) 3F 2 (过量) +Cl 2 ===2ClF 3 (ClF 3 +3H 2 O==3HF+HClO 3 ) Cl 2 +H 2 2HCl (将 H 2 在 Cl 2 点燃;混合点燃、加热、光照发生爆炸) 3Cl 2 +2P 2PCl 3 Cl 2 +PCl 3 PCl 5 Cl 2 +2Na 2NaCl 3Cl 2 +2Fe 2FeCl 3 Cl 2 +Cu CuCl 2 Cl 2 +2FeCl 2 ===2FeCl 3 (在水溶液中:Cl 2 +2Fe 2+ ===2Fe 3+ +3Cl) Cl 2 +2NaBr===2NaCl+Br 2 Cl 2 +2Br=2Cl+Br 2 Cl 2 +2KI===2KCl+I 2 Cl 2 +2I=2Cl+I 2 3Cl 2 (过量) +2KI+3H 2 O===6HCl+KIO 3 3Cl 2 +I– +3H2 O=6H+ +6Cl – +IO3– 5Cl 2 +I 2 +6H 2 O===2HIO 3 +10HCl 5Cl 2 +I 2 +6H 2 O=10Cl– +IO3– +12H + Cl 2 +Na 2 S===2NaCl+S↓ Cl 2 +S 2– =2Cl – +S ↓ Cl 2 +H 2 S===2HCl+S↓ (水溶液中:Cl 2 +H 2 S=2H + +2Cl– +S ↓ Cl 2 +SO 2 +2H 2 O===H 2 SO 4 +2HCl Cl 2 +SO 2 +2H 2 O=4H + +SO 4 2– +2Cl – Cl 2 +H 2 O 2 ===2HCl+O 2 Cl 2 +H 2 O 2 =2H + +Cl– +O2 2O 2 +3Fe Fe 3 O 4 O 2 +K===KO 2 S+H 2 H 2 S 2S+C CS 2 S+Zn ZnS S+Fe FeS (既能由单质制取,又能由离子制取) S+2Cu Cu 2 S (只能由单质制取,不能由离子制取) 3S+2Al Al 2 S 3 (只能由单质制取,不能由离子制取) N 2 +3H 2 催化剂 高温高压 2NH 3 N 2 +3Mg Mg 3 N 2 N 2 +3Ca Ca 3 N 2 N 2 +3Ba Ba 3 N 2 N 2 +6Na 2Na 3 N N 2 +6K 2K 3 N N 2 +6Rb 2Rb 3 N N 2 +2Al 2AlN P 4 +6H 2 4PH 3 P+3Na Na 3 P 2P+3Zn Zn 3 P 2 H 2 +2Li 2 LiH 2、还原性 S+O 2 SO 2 S+H 2 SO 4 (浓) 3SO 2 ↑+2H 2 O S+6HNO 3 (浓) H 2 SO 4 +6NO 2 ↑+2H 2 O S+4H + +6==6NO 2 ↑ ↑+2H 2 O+- 24SO 3S+4HNO 3 (稀) 3SO 2 +4NO↑+2H 2 O 3S+4H + +43NO 3SO 2 +4NO ↑+2H 2 O N 2 +O 2 2NO 4P+5O 2 P 4 O 10 (常写成 P 2 O 5 ) 2P+3X 2 2PX 3 (X 表示 F 2 ,Cl 2 ,Br 2 ) PX 3 +X 2 PX 5 P 4 +20HNO 3 (浓) 4H 3 PO 4 +20NO 2 ↑+4H 2 O C+2F 2 CF 4 C+2Cl 2 CCl 4 C+O 2 (足量) CO 2 2C+O 2 (少量) 2CO C+CO 2 2CO C+H 2 O CO+H 2 (生成水煤气) 2C+SiO 2 Si+2CO(制得粗硅) Si(粗)+2Cl 2 SiCl 4 (SiCl 4 +2H 2 ===Si(纯)+4HCl) Si(粉)+O 2 SiO 2 Si+C SiC(金刚砂) Si+2NaOH+H 2 O==Na 2 SiO 3 +2H 2 ↑ (Si+2OH+H 2 O= 23SiO +2H 2 ↑ ↑) 3、歧化反应 Cl 2 +H 2 O==HCl+HClO(加碱或光照促进歧化: (Cl 2 +H 2 O H + +Cl– +HClO ) Cl 2 +2NaOH==NaCl+NaClO+H 2 O (Cl 2 +2OH– =Cl – +ClO – +H2 O) Cl 2 +2Ca(OH) 2 ==CaCl 2 +Ca(ClO) 2 +2H 2 O (Cl 2 +2OH– =Cl – +ClO – +H2 O) 3Cl 2 +6KOH (浓) 5KCl+KClO 3 +3H 2 O (3Cl 2 +6OH–5Cl– +ClO3– +3H2 O) 3S+6NaOH 2Na 2 S+Na 2 SO 3 +3H 2 O (3S+6OH–2S 2– +SO32 – +3H2 O) 4P+3KOH (浓) +3H 2 O==PH 3 ↑+3KH 2 PO 2 (4P+3OH– +3H2 O==PH 3 ↑↑+3H 2 PO 2– ) 11P+15CuSO 4 +24H 2 O==5Cu 3 P+6H 3 PO 4 +15H 2 SO 4 3C+CaO CaC 2 +CO↑ 3C+SiO 2 SiC+2CO↑ 二.金属单质(Na,Mg,Al,Fe,Cu)的还原性 2Na+H 2 2NaH 4Na+O 2 ==2Na 2 O 2Na 2 O+O 2 2Na 2 O 2 2Na+O 2 Na 2 O 2 2Na+S==Na 2 S(爆炸) 2Na+2H 2 O==2NaOH+H 2 ↑ 2Na+2H 2 O=2Na + +2OH― +H2 ↑↑ 2Na+2NH 3 ==2NaNH 2 +H 2 ↑ 2Na+2NH 3 =2Na + +2NH 2― +H2 ↑↑ 4Na+TiCl 4 4NaCl+Ti Mg+Cl 2MgCl 2 Mg+Br 2 MgBr 2 2Mg+O 2 2MgO Mg+S MgS 2Cu+S Cu 2 S (Cu 2 S 只能由单质制备) Mg+2H 2 O Mg(OH) 2 +H 2 ↑ 2Mg+TiCl 4 Ti+2MgCl 2 Mg+2RbCl MgCl 2 +2Rb 2Mg+CO 2 2MgO+C 2Mg+SiO 2 2MgO+Si Mg+H 2 S==MgS+H 2 Mg+H 2 SO 4 ==MgSO 4 +H 2 ↑ ( (Mg+2H + =Mg 2+ +H 2 ↑ ↑) ) 2Al+3Cl 2 2AlCl 3 4Al+3O 2 ===2Al 2 O 3 (常温生成致密氧化膜而钝化,在氧气中燃烧) 4Al(Hg)+3O 2 +2xH 2 O===2(Al 2 O 3 .xH 2 O)+4Hg(铝汞齐) 4Al+3MnO 2 2Al 2 O 3 +3Mn 2Al+Cr 2 O 3 Al 2 O 3 +2Cr (铝热反应) 2Al+Fe 2 O 3 Al 2 O 3 +2Fe 2Al+3FeO Al 2 O 3 +3Fe 2Al+6HCl===2AlCl 3 +3H 2 ↑ 2Al+6H + =2Al 3+ +3H 2 ↑ ↑ 2Al+3H 2 SO 4 ===Al 2 (SO 4 ) 3 +3H 2 ↑ 2Al+6H + =2Al 3+ +3H 2 ↑ ↑ 2Al+6H 2 SO 4 (浓)===Al 2 (SO 4 ) 3 +3SO 2 +6H 2 O (Al,Fe 在冷,浓的 H 2 SO 4 ,HNO 3 中钝化) Al+4HNO 3 (稀)===Al(NO 3 ) 3 +NO↑+2H 2 O Al+4H + +NO 3– =Al 3+ +NO ↑+2H 2 O 2Al+2NaOH+2H 2 O===2NaAlO 2 +3H 2 ↑ 2Al+2OH– +2H2 O=2AlO 2– +3H2 ↑↑ 2Fe+3Br 2 ===2FeBr 3 3Fe+2O 2 Fe 3 O 4 2Fe+O 2 2FeO (炼钢过程) Fe+I 2 FeI 2 Fe+S FeS (FeS 既能由单质制备,又能由离子制备) 3Fe+4H 2 O(g) Fe 3 O 4 +4H 2 ↑ Fe+2HCl===FeCl 2 +H 2 ↑ Fe+2H + =Fe 2+ +H 2 ↑ ↑ Fe+CuCl 2 ===FeCl 2 +Cu Fe+Cu 2+ =Fe 2+ +Cu ↓ Fe+SnCl 4 ===FeCl 2 +SnCl 2 (铁在酸性环境下,不能把四氯化锡完全还原为单质锡Fe+SnCl 2 ==FeCl 2 +Sn↓ Fe+Sn 2+ =Fe 2+ +Sn ↓ 三.非金属氢化物(HF,HCl,H 2 O,H 2 S,NH 3 ) 金属氢化物(NaH) 1、还原性: 4HCl(浓)+MnO 2 MnCl 2 +Cl 2 ↑+2H 2 O 4H + +2Cl– +MnO2Mn 2+ +Cl 2 ↑ ↑+2H 2 O 4HCl(浓)+PbO 2 PbCl 2 +Cl 2 ↑+2H 2 O 4H + +2Cl– +PbO2Pb 2+ +Cl 2 ↑ ↑+2H 2 O 4HCl(g)+O 2 2Cl 2 +2H 2 O 16HCl+2KMnO 4 ===2KCl+2MnCl 2 +5Cl 2 ↑+8H 2 O 16 H + +10Cl- - +2MnO4– =2Mn 2+ +5Cl2 ↑↑+8H 2 O 6HCl+KClO 3 ==KCl+3Cl 2 ↑+3H 2 O 6H + +5Cl– +ClO3– =3Cl2 ↑↑+3H 2 O 14HCl+K 2 Cr 2 O 7 ===2KCl+2CrCl 3 +3Cl 2 ↑+7H 2 O 14H + +6Cl– +Cr2 O 72 – =2Cr 3+ +5Cl2 ↑↑+7H 2 O 2H 2 O+2F 2 ===4HF+O 2 2HCl+F 2 =2HF+Cl 2 (F 2 气与 HCl、HBr、HI、H 2 S、NH 3 气体不能共存) 2HBr+Cl 2 =2HCl+Br 2 (Cl 2 气与 HBr、HI、H 2 S、NH 3 气体不能共存) 2H 2 S+3O 2 (足量) 2SO 2 +2H 2 O 2H 2 S+O 2 (少量) 2S↓+2H 2 O 2H 2 S+SO 2 ===3S↓+2H 2 O H 2 S+H 2 SO 4 (浓) ===S↓+SO 2 ↑+2H 2 O 3H 2 S+2HNO 3 (稀) ===3S↓+2NO↑+4H 2 O 3H 2 S+2H + +2NO 3– =3S ↓+2NO ↑+4H 2 O 5H 2 S+2KMnO 4 +3H 2 SO 4 ===2MnSO 4 +K 2 SO 4 +5S↓+8H 2 O 5H 2 S+2MnO 4– +6H + =2Mn 2+ +5S ↓+8H 2 O 3H 2 S+K 2 Cr 2 O 7 +4H 2 SO 4 ===Cr 2 (SO 4 ) 3 +K 2 SO 4 +3S↓+7H 2 O 3H 2 S+Cr 2 O 7 2– +8H + ===2Cr 3+ +3S ↓+7H 2 O H 2 S+4Na 2 O 2 +2H 2 O===Na 2 SO 4 +6NaOH H 2 S+4Na 2 O 2 +2H 2 O=8Na + + 24SO +OH 2NH 3 +3CuO 3Cu+N 2 +3H 2 O 2NH 3 +3Cl 2 ===N 2 +6HCl 8NH 3 +3Cl 2 ===N 2 +6NH 4 Cl NH 3 +NaNO 2 +HCl==NaCl+N 2 ↑+2H 2 O NH 3 +NO 2– +H + =N2 ↑↑+2H 2 O 4NH 3 +3O 2 (纯氧) 2N 2 +6H 2 O 4NH 3 +5O 2 催化剂 △ 4NO+6H 2 O 4NH 3 +6NO===5N 2 +6H 2 O (用氨清除 NO) NaH+H 2 O===NaOH+H 2 ↑ (生氢剂) NaH+H 2 O=Na + +OH– +H2 ↑↑ 4NaH+TiCl 4 Ti+4NaCl+2H 2 ↑ CaH 2 +2H 2 O=Ca(OH) 2 ↓+2H 2 ↑ 2、酸性: 4HF+SiO 2 ===SiF 4 +2H 2 O(可测定矿样或钢样中 SiO 2 的含量,玻璃雕刻) 4HF+Si===SiF 4 +2H 2 ↑ 2HF+CaCl 2 ===CaF 2 +2HCl H 2 S+Fe===FeS↓+H 2 ↑ H 2 S+CuCl 2 ===CuS↓+2HCl (弱酸制强酸的典型反应) H 2 S+Cu 2+ =CuS ↓+2H + H 2 S+2AgNO 3 ===Ag 2 S↓+2HNO 3 H 2 S+2Ag + =Ag 2 S ↓+2H + H 2 S+HgCl 2 ===HgS↓+2HCl H 2 S+Hg 2+ =HgS ↓+2H + H 2 S+Pb(NO 3 ) 2 ===PbS↓+2HNO 3 (铅试纸检验空气中 H 2 S) H 2 S+Pb 2+ =PbS ↓+2H + H 2 S+2Ag===Ag 2 S+H 2 ↑(银器在空气中变黑的原因) 2NH 3 (液) +2Na==2NaNH 2 +H 2 ↑ (NaNH 2 +H 2 O===NaOH+NH 3 ↑) 3、NH 3 的碱性: NH 3 +HX===NH 4 X (X:F、Cl、Br、I、S) NH 3 +HNO 3 ===NH 4 NO 3 NH 3 +H + =NH 4 + 2NH 3 +H 2 SO 4 ===(NH 4 ) 2 SO 4 NH 3 +H + =NH 4 + NH 3 +NaCl+H 2 O+CO 2 ===NaHCO 3 +NH 4 Cl(侯德榜制碱:用于工业制备小苏打,苏打) NH 3 +H 2 S==NH 4 HS NH 3 +H 2 S=NH 4 + + HS- 4、不稳定性: 2HF H 2 +F 2 2HCl H 2 +Cl 2 2H 2 O 2H 2 +O 2 2H 2 O 2 ===2H 2 O+O 2 H 2 S H 2 +S 2NH 3 催化剂 N 2 +3H 2 2HI H 2 +I 2 四.非金属氧化物(SO 3 、SO 2 、N 2 O、NO、N 2 O 3 、NO 2 、N 2 O 4 、N 2 O 5 、CO、CO 2 、SiO 2 、P 2 O 3 、P 2 O 5 、Cl 2 O、Cl 2 O 3 、Cl 2 O 5 、Cl 2 O 7 、ClO 2 ) 1、低价态的还原性:(SO 2 、CO、NO) 2SO 2 +O 2 +2H 2 O===2H 2 SO 4 (这是 SO 2 在大气中缓慢发生的环境化学反应) 2SO 2 +O 2 催化剂 加热 2SO 3 SO 2 +NO 2 ===SO 3 +NO SO 2 +Cl 2 +2H 2 O===H 2 SO 4 +2HCl Cl 2 +SO 2 +2H 2 O=4H + +SO 4 2– +2Cl – SO 2 +Br 2 +2H 2 O===H 2 SO 4 +2HBr Br 2 +SO 2 +2H 2 O=4H + +SO 4 2– +2Br – SO 2 +I 2 +2H 2 O===H 2 SO 4 +2HI I 2 +SO 2 +2H 2 O=4H + +SO 4 2– +2I – 2NO+O 2 ===2NO 2 NO+NO 2 +2NaOH===2NaNO 2 (用于制硝酸工业中吸收尾气中的 NO 和 NO 2 ) NO+NO 2 +2OH– =2NO2– 2CO+O 2 2CO 2 CO+CuO Cu+CO 2 3CO+Fe 2 O 3 2Fe+3CO 2 CO+H 2 O 催化剂 加热 CO 2 +H 2 2、氧化性: SO 2 +2H 2 S===3S+2H 2 O SO 3 +2KI K 2 SO 3 +I 2 NO 2 +2KI+H 2 O===NO+I 2 +2KOH(不能用淀粉 KI 溶液鉴别溴蒸气和 NO 2 ) 4NO 2 +H 2 S===4NO+SO 3 +H 2 O 2NO 2 +Cu 4CuO+N 2 N 2 O+Zn ZnO+N 2 CO 2 +2Mg 2MgO+C (CO 2 不能用于扑灭由 Mg,Ca,Ba,Na,K 等燃烧的火灾) SiO 2 +2H 2 Si+2H 2 O SiO 2 +2Mg 2MgO+Si 3、与水的作用: SO 2 +H 2 O===H 2 SO 3 SO 3 +H 2 O===H 2 SO 4 SO 3 +H 2 O=2H + +SO 4 2– 3NO 2 +H 2 O===2HNO 3 +NO (NO 2 不是硝酸的酸酐) N 2 O 5 +H 2 O===2HNO 3 N 2 O 5 +H 2 O=2H + +2NO 3– P 2 O 5 +H 2 O(冷水)===2HPO 3 P 2 O 5 +3H 2 O(热水)===2H 3 PO 4 (P 2 O5 极易吸水,可作气体干燥剂) P 2 O 5 +3H 2 SO 4 (浓)===2H 3 PO 4 +3SO 3 CO 2 +H 2 O===H 2 CO 3 Cl 2 O+H 2 O==2HClO Cl 2 O 7 +H 2 O==2HClO 4 Cl 2 O 7 +H 2 O=2H + +2ClO 4– 4、与碱性物质的作用: SO 2 +2NH 3 +H 2 O===(NH 4 ) 2 SO 3 SO 2 +(NH 4 ) 2 SO 3 +H 2 O===2NH 4 HSO 3 2NH 4 HSO 3 +H 2 SO 4 ===(NH 4 ) 2 SO 4 +2H 2 O+2SO 2 ↑(硫酸工业尾气处理) SO 2 +Ca(OH) 2 ===CaSO 3 ↓+H 2 O (不能用澄清石灰水鉴别 SO 2 和 CO 2 .可用品红鉴别) SO 3 +MgO===MgSO 4 SO 3 +Ca(OH) 2 ===CaSO 4 ↓+H 2 O CO 2 +NH 3 +H 2 O===NH 4 HCO 3 CO 2 +2NH 3 (过量) +H 2 O===(NH 4 ) 2 CO 3 (NH 4 ) 2 CO 3 (NH 2 ) 2 CO+2H 2 O CO 2 +2NH 3 (NH 2 ) 2 CO+H 2 O (工业制取尿素) CO 2 +2NaOH (过量) ==Na 2 CO 3 +H 2 O 2OH- - +CO2 =CO 32 – +H2 O CO 2 (过量) +NaOH==NaHCO 3 OH- - +CO2 =HCO 3– CO 2 +Ca(OH) 2 (过量) ==CaCO 3 +H 2 O Ca 2+ +2OH +CO 2 =CaCO 3 ↓ ↓+H 2 O 2CO 2 (过量) +Ca(OH) 2 ==Ca(HCO 3 ) 2 OH― +CO2 =HCO 3– CO 2 +CaCO 3 +H 2 O==Ca(HCO 3 ) 2 CO 2 +CaCO 3 +H 2 O=Ca 2+ +2HCO 3– CO 2 ( 不足 )+2NaAlO 2 +3H 2 O===2Al(OH) 3 ↓+Na 2 CO 3 CO 2 +3H 2 O+AlO 2– =Al(OH)3 ↓↓+CO 3 2– CO 2 ( 足 )+NaAlO 2 +2H 2 O===Al(OH) 3 ↓+NaHCO 3 CO 2 +2H 2 O+AlO 2– =Al(OH)3 ↓↓+HCO 3– CO 2 +C 6 H 5 ONa+H 2 O===C 6 H 5 OH↓+NaHCO 3 CO 2 +C 6 H 5 O― +H2 O=C 6 H 5 OH ↓+HCO 3– SiO 2 +CaO CaSiO 3 (炼钢造渣) SiO 2 +2NaOH===Na 2 SiO 3 +H 2 O(常温下强碱缓慢腐蚀玻璃) SiO 2 +Na 2 CO 3 Na 2 SiO 3 +CO 2 (制取玻璃) SiO 2 +CaCO 3 CaSiO 3 +CO 2 (制取玻璃) 2NO 2 +2NaOH==NaNO 2 +NaNO 3 +H 2 ...