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- Page 17 and 18: 1.1 QUÍMICA: O QUE, POR QUE E COMO
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- Page 33 and 34: 1.5 A ENERGIA A energia, como a mat
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- Page 63 and 64: 1.27 Converta cada uma das seguinte
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- Page 77 and 78: 1 átomo de S: Massa = 1 x 32,1 u =
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Problema Paralelo: 8,96 x 10 21 mol
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A massa molecular do SO2 é 32,1 +
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C4H5. Generated by Foxit PDF Creato
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Uma vez identificado o reagente lim
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Se 1,0 L de uma solução foi prepa
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Figura 2.5 o uso de um balão volum
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Note que em um problema de diluiç
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denominamos ponto de equivalência,
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2.9 O MOL: COMENTÁRIOS ADICIONAIS
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Compostos Binários Não-Metal-Não
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(a) 1 mol de átomos de Cl, (b) 1 m
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2.15 Uma amostra de um certo compos
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* 2.27 Análise de clorato de potá
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* 2.36 Quantos gramas de NH3 podem
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2.44 Escreva uma fórmula para cada
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(a) NaOH (b) Ca(OH)2 (c)Al(OH)3 (d)
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2.69 Se 1,97g de um composto consis
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3.1 APRIMEIRA LEI DA TERMODINÂMICA
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classificar todas as formas de ener
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Quando um mol de gelo funde a uma a
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eação, ele realiza um trabalho de
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caso: J °C mol Nota: É comum escr
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Problema Paralelo: Um pedaço de co
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3.4 AS EQUAÇÕES TERMOQUÍMICAS Po
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Comentários Adicionais Por que a s
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Se invertermos as primeiras duas eq
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Os carvões são classificados toma
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também à transferência de calor
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3.4 Por que ΔU e ΔH são aproxima
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3.18 A 25 °C o calor-padrão molar
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4.1 VARIÁVEIS USADAS PARA DESCREVE
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Se o nível de mercúrio no tubo do
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Diminuindo a pressão pelo fator de
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Comentários Adicionais A lei de Bo
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não é uma entidade verdadeira, as
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CÁLCULOS COMBINADOS A mesma aborda
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Problema Paralelo Uma amostra de 14
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PRINCÍPIO DE AVOGADRO Por que a re
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VOLUME MOLAR DE UM GÁS IDEAL Utili
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A pressão parcial da água é cham
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LEI DE GRAHAM DE DIFUSÃO E EFUSÃO
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ANÁLISE DO MODELO Até que ponto o
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4.7 ESTEQUIOMETRIA DOS GASES Vimos
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O volume de CO2 a 1,00 kPa e 1198 K
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E então usar a lei do gás ideal p
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(b) Usando a equação de van der W
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escrevendo E, portanto Videal = V -
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4.13 Qual é o volume molar do gás
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(c) Se H2) e N2 são retidos em um
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solução do problema, Bohr inspiro
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* 5.14 (a) Qual é a carga em coulo
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6.1 O MODELO DA MECÂNICA QUÂNTICA
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outros, tais como o sódio, Stern e
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Esse método de representação é
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7.1.) Excetuando-se o hélio, as co
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Uma análise destas configurações
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segunda camada mais externa é inte
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Como υλ = c (Seção 5.4), Portan
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6.3 AS ONDAS ESTACIONÁRIAS As onda
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Figura 6.8 O toque da corda: um seg
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Cada modo de vibração tem uma ene
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Figura 6.14 Gráfico da densidade d
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Figura 6.17 Superfícies-limites de
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Os três orbitais 2p diferem entre
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Figura 6.26 Superfícies-limites do
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6.5 OS NÚMEROS QUÂNTICOS Para den
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As Configurações Eletrônicas 6.6
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6.15 Compare, em termos de tamanho
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6.28 Descreva os nós angulares ass
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7.1 A DESCOBERTA DA LEI PERIÓDICA
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Lítio (Li, Z =3) Sódio (Na, Z = 1
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Figura 7.2 A tabela periódica dos
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Figura 7.5 A tabela periódica e a
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Tabela 7.2 Raios atômicos dos elem
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Tabela 7.4 Raios atômicos dos elem
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Figura 7.7 Primeiras energias de io
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egião extranuclear e pela adição
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Figura 7.10 Densidades dos elemento
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Os íons resultante, Fe 2+ , são c
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Este sufixo é também usado para a
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velocidade da reação geralmente a
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A PERIODICIDADE NA ESTEQUIOMETRIA A
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PROBLEMAS Histórico 7.1 Em 1829, o
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Propriedades Atômicas 7.11 Qual o
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7.24 Escreva uma equação química
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(a) FeBr3 (b) FeBr2 (c) Cr(OH)3 (d)
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8.1 LIGAÇÕES IÓNICAS A formaçã
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Um átomo de cloro possui sete elé
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Tabela 8.1 As estruturas de Lewis p
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Exemplo 8.1 Escreva a estrutura de
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chamada de energia reticular do clo
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E os dois que sobram formam um par
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eletronegatividades (os elementos m
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Figura 8.9 As eletronegatividades d
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Tabela 8.3 Energias de ligação (k
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Solução: A reação pode ser subd
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Exemplo 8.10 Atribua a carga formal
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Figura 8.13 A molécula de AsCl3: p
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Exemplo 8.11 Faça uma previsão da
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Figura 8.18 A molécula de ClF3. Co
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A situação é diferente na moléc
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Considere agora a molécula da águ
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8.7 Cada uma das seguintes molécul
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Figura 9.1 Um monocristal de quartz
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Figura 9.3 Difração de raios X pe
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produzidos na "ampliação", verifi
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Uma rede é um arranjo regular, rep
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O Cloreto de Sódio. Em sólidos i
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Figura 9.24 A estrutura da fluorita
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9.5 LIGAÇÕES E PROPRIEDADES DOS S
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atração entre os átomos. A atra
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iônicos, não sendo satisfatório
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PROBLEMAS Sólidos: Considerações
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10.1 LÍQUIDOS Propriedades gerais
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tornando-se maior com a temperatura
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Esta é a forma geral da equação
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Portanto, Problema Paralelo: Usando
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em equilíbrio. Embora neste capít
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651 Apêndice A GLOSSÁRIO DE TERMO
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655 Cetona.Composto orgânico do ti
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661 Equivalente (redox). A quantida
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663 Grupo carbonila. A estrutura Gr
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665 Ligação covalente não-polar.
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667 Molécula polar. Molécula na q
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671 Polimorfismo. A habilidade de u
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675 Solução supersaturada. Soluç
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677 Viscosidade. A resistência ao
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B.2 CONSTANTES FÍSICAS 681 Generat
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CÁTIONS CÁTIONS MONOATÔMICOS Qua
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CÁTIONS POLIATÔMICOS Cátions com
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Os sufixos -ito e -ato são usados
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691 Tabela C.4 Nomes de alguns âni
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ÓXIDOS Os óxidos de metais são d
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OUTROS COMPOSTOS INORGÂNICOS Muito
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Ligantes Neutros. O nome de uma mol
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SAIS CONTENDO ÍONS COMPLEXOS Para
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Os prefixos di-, tri-, tetra- etc.,
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DERIVADOS DE HIDROCARBONETOS Alguns
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707 Agora suponha que num segundo e
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709 logaritmo natural de N = loge N
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Note que cada estrutura usa todos o
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H.3 PRODUTOS DE SOLUBILIDADE 723 Ge
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727 Apêndice I POTENCIAIS DE REDU
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731 Apêndice J RESPOSTAS DOS PROBL
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