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Universities » Wake Forest University (WF) » CHM - Chemistry » 111 - College Chemistry I » Flash Cards

Reactions / Electromagnetic - Flashcards

Flashcard Deck Information

Class:	CHM 111 - College Chemistry I
Subject:	Chemistry
University:	Wake Forest University
Term:	Fall 2010

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Electrolytes

substance which dissolves in water to produce conducting solutions (cation+anion)
(breaks into ions)

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weak electrolytes: defn

compounds that dissociate to a small extent into ions when dissolved in water (usually have a double arrow)

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Strong electrolytes: list

HCl, HBr, HI, HClO4, HNO3, H2SO4, KBr, KI, NaCl, NaOH, KOH,.. (all ionic compounds)

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weak electrolytes: list

CH3CO2H, HF, HC2H3O2 (Acetic acid)

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non electrolytes: list

H2O, CH3OH (menthyl alcohol), C2H5OH (ethyl alcohol), C12H22O11 (sucrose), and most carbon compounds (molecular compounds

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acid

compound that can donate H+. You can recognize acid formulas as those that start with H or end with COOH. ( i.e HNO3 and HCOOH)

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base

is a compound that can accept H+. Base formulas often contain a metal cation with the hydroxide anion, OH-. Bases that do not contain OH usually contain N. (i.e NaOH and NH3)

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salt

an ionic compound that is neither an acid nor a base. To identify a salt, look for a formula that contains a cation that is not H+ and an anion that is not OH-. (i.e NaBr and KCl)

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anion

gains e- which makes it negative in charge (anion is written as SO2−4, the "2−" indicating that it has two more electrons than it has protons)

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cation

loses e- ( i.e. Na+)

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Insoluble list :CHOPS

carbonates (CO3 2-), hydroxides (OH-), oxalates (C2O4 2-), phosphates (PO4 3-), sulfides (S 2-)

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Exceptions to the insoluble

insoluble except ionic compound with group 1A and NH4+

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Sulfide solubility

insoluble except with group 1A, NH4+, and group 2A (Mg, Ca, Ba are sparingly soluble)

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Hydroxide solubility

all hyrdoxides are insoluble except those of NH4+ and Group 1A, and (SrOH2, BaOH2, CaOH2)

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oxidation

loss of one or more electrons,

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reduction

gain of one or more electrons

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reducing agent

causes reduction, loses on or more electrons , undergoes oxidation, oxidation number of atom INCREASES

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oxidizing agent

causes oxidation, gains one ore more electrons, undergoes reduction, oxidation number of atom DECREASES

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de broglie wavelength

wavelength = h/mv = h/mc=c/v=hc/E

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blamer series

2nd shell; if excited e- drops to second shell then light emitted will be in the Balmer series

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Principal quantum number (n)

"n", describes the size and E level of the orbital (shell), eqn "2n^2"

as n increases the distance from the nucleus increases and the E of the electrons increases

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angular momentum quantum number aka spherical orbital (l)

"l" , the subshell, ranges from 0 to (n-1), number of nodes

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subshell notation (l)

l=0=s , 1=p, 2=d, 3=f

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magnetic quantum number (m_l)

"m_l" , (2l+1) ranges from -l to +l

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spin quantum number (m_s)

+1/2 or -1/2

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pauli exclusion

no two e-s can have the same spin, no two e-'s can have the same four quantum numbers

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aufbau principle

lower orbitals fill before higher e- orbitals, e-'s are removed first from the valence shell

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hund's rule

unpaired e- fill first

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antiparallel

electrons with opposite spins

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diamagnetic

a substance with paired electrons is repelled by a magnetic field

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Electrolytes	substance which dissolves in water to produce conducting solutions (cation+anion) (breaks into ions)
weak electrolytes: defn	compounds that dissociate to a small extent into ions when dissolved in water (usually have a double arrow)
Strong electrolytes: list	HCl, HBr, HI, HClO4, HNO3, H2SO4, KBr, KI, NaCl, NaOH, KOH,.. (all ionic compounds)
weak electrolytes: list	CH3CO2H, HF, HC2H3O2 (Acetic acid)

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non electrolytes: list	H2O, CH3OH (menthyl alcohol), C2H5OH (ethyl alcohol), C12H22O11 (sucrose), and most carbon compounds (molecular compounds
acid	compound that can donate H+. You can recognize acid formulas as those that start with H or end with COOH. ( i.e HNO3 and HCOOH)
base	is a compound that can accept H+. Base formulas often contain a metal cation with the hydroxide anion, OH-. Bases that do not contain OH usually contain N. (i.e NaOH and NH3)
salt	an ionic compound that is neither an acid nor a base. To identify a salt, look for a formula that contains a cation that is not H+ and an anion that is not OH-. (i.e NaBr and KCl)

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anion	gains e- which makes it negative in charge (anion is written as SO2−4, the "2−" indicating that it has two more electrons than it has protons)
cation	loses e- ( i.e. Na+)
Insoluble list :CHOPS	carbonates (CO3 2-), hydroxides (OH-), oxalates (C2O4 2-), phosphates (PO4 3-), sulfides (S 2-)
Exceptions to the insoluble	insoluble except ionic compound with group 1A and NH4+

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Sulfide solubility	insoluble except with group 1A, NH4+, and group 2A (Mg, Ca, Ba are sparingly soluble)
Hydroxide solubility	all hyrdoxides are insoluble except those of NH4+ and Group 1A, and (SrOH2, BaOH2, CaOH2)
oxidation	loss of one or more electrons,
reduction	gain of one or more electrons

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reducing agent	causes reduction, loses on or more electrons , undergoes oxidation, oxidation number of atom INCREASES
oxidizing agent	causes oxidation, gains one ore more electrons, undergoes reduction, oxidation number of atom DECREASES
de broglie wavelength	wavelength = h/mv = h/mc=c/v=hc/E
blamer series	2nd shell; if excited e- drops to second shell then light emitted will be in the Balmer series

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Principal quantum number (n)	"n", describes the size and E level of the orbital (shell), eqn "2n^2" as n increases the distance from the nucleus increases and the E of the electrons increases
angular momentum quantum number aka spherical orbital (l)	"l" , the subshell, ranges from 0 to (n-1), number of nodes
subshell notation (l)	l=0=s , 1=p, 2=d, 3=f
magnetic quantum number (m_l)	"m_l" , (2l+1) ranges from -l to +l

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spin quantum number (m_s)	+1/2 or -1/2
pauli exclusion	no two e-s can have the same spin, no two e-'s can have the same four quantum numbers
aufbau principle	lower orbitals fill before higher e- orbitals, e-'s are removed first from the valence shell
hund's rule	unpaired e- fill first

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antiparallel	electrons with opposite spins
diamagnetic	a substance with paired electrons is repelled by a magnetic field

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List View: Terms & Definitions

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	Front	Back
	Electrolytes	substance which dissolves in water to produce conducting solutions (cation+anion) (breaks into ions)
	weak electrolytes: defn	compounds that dissociate to a small extent into ions when dissolved in water (usually have a double arrow)
	Strong electrolytes: list	HCl, HBr, HI, HClO4, HNO3, H2SO4, KBr, KI, NaCl, NaOH, KOH,.. (all ionic compounds)
	weak electrolytes: list	CH3CO2H, HF, HC2H3O2 (Acetic acid)
	non electrolytes: list	H2O, CH3OH (menthyl alcohol), C2H5OH (ethyl alcohol), C12H22O11 (sucrose), and most carbon compounds (molecular compounds
	acid	compound that can donate H+. You can recognize acid formulas as those that start with H or end with COOH. ( i.e HNO3 and HCOOH)
	base	is a compound that can accept H+. Base formulas often contain a metal cation with the hydroxide anion, OH-. Bases that do not contain OH usually contain N. (i.e NaOH and NH3)
	salt	an ionic compound that is neither an acid nor a base. To identify a salt, look for a formula that contains a cation that is not H+ and an anion that is not OH-. (i.e NaBr and KCl)
	anion	gains e- which makes it negative in charge (anion is written as SO2−4, the "2−" indicating that it has two more electrons than it has protons)
	cation	loses e- ( i.e. Na+)
	Insoluble list :CHOPS	carbonates (CO3 2-), hydroxides (OH-), oxalates (C2O4 2-), phosphates (PO4 3-), sulfides (S 2-)
	Exceptions to the insoluble	insoluble except ionic compound with group 1A and NH4+
	Sulfide solubility	insoluble except with group 1A, NH4+, and group 2A (Mg, Ca, Ba are sparingly soluble)
	Hydroxide solubility	all hyrdoxides are insoluble except those of NH4+ and Group 1A, and (SrOH2, BaOH2, CaOH2)
	oxidation	loss of one or more electrons,
	reduction	gain of one or more electrons
	reducing agent	causes reduction, loses on or more electrons , undergoes oxidation, oxidation number of atom INCREASES
	oxidizing agent	causes oxidation, gains one ore more electrons, undergoes reduction, oxidation number of atom DECREASES
	de broglie wavelength	wavelength = h/mv = h/mc=c/v=hc/E
	blamer series	2nd shell; if excited e- drops to second shell then light emitted will be in the Balmer series
	Principal quantum number (n)	"n", describes the size and E level of the orbital (shell), eqn "2n^2" as n increases the distance from the nucleus increases and the E of the electrons increases
	angular momentum quantum number aka spherical orbital (l)	"l" , the subshell, ranges from 0 to (n-1), number of nodes
	subshell notation (l)	l=0=s , 1=p, 2=d, 3=f
	magnetic quantum number (m_l)	"m_l" , (2l+1) ranges from -l to +l
	spin quantum number (m_s)	+1/2 or -1/2
	pauli exclusion	no two e-s can have the same spin, no two e-'s can have the same four quantum numbers
	aufbau principle	lower orbitals fill before higher e- orbitals, e-'s are removed first from the valence shell
	hund's rule	unpaired e- fill first
	antiparallel	electrons with opposite spins
	diamagnetic	a substance with paired electrons is repelled by a magnetic field

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