Chapter 1 Structure and Bonding Flashcards

1
Q

What is an atom

A

an atom consists of a dense, positively charged nucleus surrounded at a relatively large distance by negatively charged electrons.

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2
Q

What is a nucleus

A

Nucleus consists of subatomic particles called neutrons, which are electrically neutral, and protons, which are positively charged.

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3
Q

Atomic Number (Z)

A

Gives the number of protons or an atom contains.

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4
Q

Mass number (A)

A

which gives the total number of protons and neutrons in its nucleus.

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5
Q

Isotopes

A

Atoms with the same atomic number but different mass numbers are called? Neutrons can change.

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6
Q

Atomic Weight

A

The weighted-average of an element’s naturally occurring isotopes is called…..

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7
Q

Node

A

A region of zero electron density around the nucleus.

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8
Q

Atomic Orbital

A

A mathematically defined 3D region of space around a nucleus where an electron spends its time.

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9
Q

Electron Cloud

A

made from electrons relatively small and contain 1- charge, determines volume of an atom.

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10
Q

Electron shell

A

The orbitals in an atom are organized into different layers around the nucleus called….

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11
Q

Aufbau principle

A

The lowest-energy orbitals fill up first, 1S->2S->2P->3S

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12
Q

Pauli exclusion principle

A

Only two electrons can occupy an orbital, and they must have opposite spins.

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13
Q

Hund’s Rule

A

If two or more empty orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half-full.

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14
Q

Covalent bond

A

shared electron bond not by gaining or losing electrons, but by sharing them.

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15
Q

Molecule

A

The neutral collection of atoms held together by covalent bonds.

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16
Q

Lewis structures/ Electron-dot structures

A

the valence-shell electrons of an atom are represented as dots. A stable molecule results whenever a noble-gas configuration of eight dots and octet is achieved.

17
Q

Kekule structures/ line-bond structures

A

two-electron covalent bonds are indicated as lines drawn between atoms.

18
Q

Lone-pair electrons/ nonbonding electrons

A

Valence electrons that are not used for bonding remain as dots in structures are called….

19
Q

Valence bond theory

A

a covalent bond forms when two atoms approach each other closely and a singly occupied orbital on one atom overlaps a singly occupied orbital on the other atom.

20
Q

Sigma Bonds (σ)

A

Bonds which are formed by the head-on overlap of two atomic orbitals along a line drawn between the neclei. Increased electron density in middle between atoms.

21
Q

Molecular Orbitals

A

mathmatical combination of atomic orbitals that forms so e- belong to the whole molecule.

22
Q

sp^3 orbitals

A

One 2s+3p form four new sp^3 orbitals to make for new sigma bonds. First bond between atoms is always a sigma bond and allows for free rotation. Tetrahedral geometry with 109.5 bond angles.

23
Q

sp^2 hybridization

A

one 2s+two 2p= three new sp2 orbitals. 3 sigma bond and one pi bond can be made. trigonal planar geometry with 120 bond angles.

24
Q

Pi bonds (π)

A

result from sideways overlap, relatively weak bonds, do not allow for free rotation, Pi bonds is every bond other than sigma bonds.

25
Q

Sp Hybridization

A

One 2s+one 2p= two new sp orbitals. uses two sp to make 2 sigma bonds two unchanged p orbitals used to make 2 pi bonds, linear molecule with 180 bond angles.

26
Q

Ground state electron configuration

A

assigning electrons to the proper orbitals, beginning with the lowest-energy ones

27
Q
A