- Decreases from left to right - Increases as descends

- more negative left to right - more positive most positive as descends frst column only - -no clear trend in general going down

Final Flashcards by sophia winters

effective nuclear charge (Zeff)

increases from left to right

- stays the same top to bottom(increases slightly)

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Core size

Decreases from left to right

- Increases as descends

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Electron affinity

more negative left to right
more positive most positive as descends frst column only
-no clear trend in general going down

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Melting point

GROUP 1A: Decreases as descends

Group 7A: Increases as descends

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Density

GROUP 1A: Decreases as descends

Group 7A: Increases as descends

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Metallic Characteristics

decreases from left to right

- Increases as descends

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ionization energy

-energy needed to remove an electron

Increases from left to right

- Decreases as descends

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Halogens with respect to electron affinity

very exothermic electron affinity values
-electron affinity values are more negative for elements that prefer to gain, rather than lose, an electron (negative ions)

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boiling part for group 7A

-increase as descends

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what is true regarding ionization energies

they are all endothermic

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Elements have a series of ionization energies for removing the first and additional electrons from the atom. Each ionization energy increases for successive electrons being removed. Where will the largest jump in ionization energies occur for aluminum?

Aluminum because it has there valence electrons so the fourth, the shell electron will be the hardest to remove

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what is the most reactive nonmetal, in fairly extremes circumstances,

fluorine

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The effective nuclear charge is the amount of charge experienced by an electron taking into account any shielding effects from other electrons. Electrons between the nucleus and the electron of interest cause shielding and reduce the actual charge felt by the electron of interest.

The outermost electron of boron experiences a lower effective nuclear charge than carbon. Why?

The nuclear charge increases from boron to carbon, but there is no additional shielding.

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what happens as you move down he rows

Higher energy levels

-more electronic shells

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what happens as you move across the columns

more electronic valence shells

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how to alkali metals react with halogens

diatomic elements that reacts vigorously with sodium metal to produce compounds for example

Br2+2Na–2BrN

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size comparison anion, cation, neutral

Anion, Neutral, Cation

Biggest——->Smallest

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How many covalent bonds are usually formed from the element F

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when is it appropriate to form double or triple bonds in a Less Structure?

when the central atom does not have an octet of electrons

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How many covalent bonds are usually formed from the element H

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How many covalent bonds usually formed by N

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How many covalent bonds usually formed by O

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How many covalent bonds are usually formed by the element C

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2 electron groups
2 bonding groups
0 lone pairs

Electron: linear
Molecular: linear
Angles: 180
Hybridization: sp

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3 electron groups 3 bonding groups 0 lone pairs

electron: trigonal planar molecular: trigonal planar angle: 120 Hybridization: sp2

3 electron groups 2 bonding groups 1 lone pair

electron: trigonal planar molecular: bent angle: <120 Hybridization: sp2

4 electron groups 4 bonding groups 0 lone pair

electron: tetrahedral molecular: tetrahedral angel: 109.5 Hybridization: sp3

4 electron groups 3 bonding groups 1 lone pair

electron: tetrahedral molecular: trigonal pyramidal angle: <109.5 Hybridization: sp3

4 electron groups 2 bonding gropus 2 lone pairs

electron: tetrahedral molecular: bent angle: <<109.5 Hybridization: sp3

5 electron groups 5 bonding groups 0 lone pairs

electron: trigonal bipyramidal Molecular: trigonal bipyramidal angle 120 equatorial 90 axial Hybridization: sp3d

5 electron groups 4 bonding groups 1 lone pair

``` electron trigonal bipyramidal molecular: seesaw ange: <120 equatorial <90 axial Hybridization: sp3d ```

5 electron groups 3 bonding groups 2 lone pairs

electron: trigonal bipyramidal molecular: t shaped angle <90 Hybridization: sp3d

5 electron groups 2 bonding groups 3 lone pairs

electron: trigonal bipyramidal molecular: linear angle 180 Hybridization: sp3d

6 electron groups 6 bonding groups 0 long pairs

electron octahedral molecular octahedral angle 90 Hybridzation: sp3d2

6 electron groups 5bonding groups 1 lone pair

electron octahedral molecular square pyramidal angle <90 Hybridzation: sp3d2

6 electron groups 4 bonding groups 2 lone pairs

electron octahedral molecular square planar angle 90 Hybridzation: sp3d2

ClF3: polar, non polar, or ionic

polar

NH3 ionic, polar, non polar

polar

Li3N ionic, polar, nonpolar

ionic

C2H4 polar, non polar, or ionic

non polar

PCl3 polar, non polar, ionic

polar

H2O polar non polar ionic

polar

Cl4C polar, non, ionic

non polar

SF6 polar, non polar, ionic

non polar

PF5 ionic, polar, non polar,

non polar

C2H3N. polar non polar ionic

polar

XeF4 ionic, polar, non polar

non polar

which element will form the most polar bond with fluorine

Boron

N2 polar, non polar, ionic

non polar

general trends in electronegativity values

increase from left to right, decrease from top to bottom

what type of intermolecular forces are found in H2CO

dispersion and dipole-dipole forces

Wha types of intermolecular forces are found in CH2Cl2

dispersion and dipole-dipole forces

London Dispersion force (LDF)

present/possible for any atom and all covalent compounds | -polar or non polar

Dipole interactions

only exist in polar covalent molecules because required to have a permanent dipole

Hydrogen bonds

special dipole-dipole meets these conditions: 1. molecule must have H in a very polar bond (H bonded to N,O,F) 2. neighbor molecules must have a N,O,F (atoms with high electronegativity and lone pairs of electrons)

Dipole bonds in liquids vs solids

Liquids: attractions and repulsions solid: only attractions

Which bonds are harder to break

those with higher boiling point and melting point, therefor a higher LDF

MW, LDF, MP, and BP, surface area, and period

``` MW increases LDF increases Boiling point Increases Melting point: increaeses More surface area Peroid decreases ```

polarizability

ability to "squash manipulate the electronic cloud

Low polaralizabeility vs high

Low= "hard" low LMF | High="soft" high LMF

CO2 polar or nonpolar

non polar

CH4 polar or non polar

non polar

what type of interaction will occur between H2O and Na+

ion-dipole forces

C+H bonded

always non polar

same ions/atoms bonded together

always non polar

BF4 polar or non polar

non polar

energy levels of bonding and antibonding orbitals?

The energy of a bonding orbital is always lower than the energy of the corresponding antibonding orbital.

Diamagnetic vs paramagnetic

Diamagnetic: all of the electrons are paired | Paramagnetic because it has unpaired electrons

What type of orbitals overlap to form the N-H bond in NH3?

sp3 of nitrogen and s of hydrogen

formula for bond order

(electrons in bonding orbitals - electrons anti bonding orbitals)/2

bond order definition

the number of chemical bonds between a pair of atoms.

the energy of a boding orbital is...

always lower than th energy of the corresponding anti bonding orbital

valence bond theory is based on the idea that

electrons in atomic or hybrid orbitals overlap to form bonds

the higher the bond order...

the more stable the bond

how are the number of standard atomic orbitals related to he number of hybrid atomic orbitals

they are equal

what is hybridization

The mathematical combination of standard atomic orbitals to form hybrid atomic orbitals where the number of standard atomic orbitals equals the number of hybrid atomic orbitals

what orbitals overlap occur to form triple bond

one sigma bond and two pi bonds

Which of the properties of a liquid are dependent on the intermolecular attractive forces in the liquid?

viscosity, surface tension, density

Final Flashcards

(78 cards)