BCH 261 Lecture Notes - Lecture 12: Nitric Acid, Ph Indicator, Hydrobromic Acid

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fairya

22 Nov 2020

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Unit 1: matter, chemical trends and chemical bonding. Atomic radius: the distance from the centre of the atom (nucleus) to the valence shell. (right to left; decreases, down; increasing) Ionization energy: energy required to remove one electron from the valence shell of a neutral atom. (left to right; increase, up; increase) Electron affinity: the amount of energy released when a neutral atom gains an electron to form a negative ion (left to right; increase, up; increase) Electronegativity: the electron attracting ability of an atom (left to right; increase, up; increase) Electron shells: electrons only exist where electron shells, or energy levels, allow them to. A difference in the number of energy levels affects the distance electrons can be from the nucleus. Nuclear charge: number of protons determines the positive charge in the nucleus. A different number of positive charges in the nucleus changes the pull on electrons. Less protons so the attraction with electrons are weaker.

Related Questions

1. True or False. a. A positively charged ion is called an anion. b. If an atom gives up an electron, it creates negatively charged ion. c. Valence electrons are the electrons that are available for bonding and located in the shells closest to the nucleus. d. An ionic bond is the result of electron sharing. e. When atoms gain, lose, or share electrons they do so in order to have an electron configuration of a noble gas. f. As you go across the periodic table left to right, electronegativity will increase. g. The number of valence electrons an atom has is equal to the atomic number. h. Fluorine cannot be the central atom due to the fact that is can only accept 2 electrons. i. When a covalent bond occurs, the atoms overlap one another to create a new orbital. The more overlapping, the stronger the bond. j. A triple bond is considered to be a weak bond.

Which of the following periodic trends is false?

a) Elements in the same column have similar reactivities because their valence electrons tend to be located in the same types of orbitals.

b) A series of ions that isoelectric (contain the same number of electrons) in their ground states have the same electron configuration.

c) The atomic size of the elements increases going across a period from left to right because the number of electrons increases, so the electrons are located further from the nucleus.

d) It takes more energy to remove an electron from lithium than from cesium because the valence electrons in lithium are located closer to the nucleus.

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BCH 261 Lecture Notes - Lecture 12: Nitric Acid, Ph Indicator, Hydrobromic Acid

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