Unit 1 - Bonding Flashcards Preview

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Flashcards in Unit 1 - Bonding Deck (35):
0

Name to formula

Take the first element and charge and then the second element and charge then balance the charges and simplify

1

Formula to name

Take the metal and then if it has two charges put the charge in brackets then the nonmetal followed by ide

2

What compounds give and receive electrons to fill their valence levels

Ionic compounds

3

What compounds share their electrons to fill their valence level

Molecular ... Covalent bonds

Also metallic

4

Two intramolecular forces (bonds in one molecule)

Covalent and ionic

5

Different Intermolecular forces (bonding of two molecules)

Dipole dipole
London dispersion
Hydrogen bonding

6

How do you draw Lewis dot diagrams ... Ionic

Take the metal and draw the electrons as dots and then the nonmetal and draw the electrons then connect the metal electrons with the nonmetal missing electrons with an arrow and then Beside it show the metal with no electrons in brackets with a negative charge of however many electrons were lost and the nonmetal with all the electrons around it and the new ones in a new colour and put a bracket around it and put a positive charge of however many electrons it gained

7

Lewis dot diagrams ... Molecular

Draw the atoms with their electrons and then make the electrons rearrange so they share the electrons there can be double or triple bonds

8

Intramolecular Forces

Bonds in a single compound. Holds together the compound.

9

Intermolecular force

Bonds between two compounds... Attractions between molecules

10

Properties of ionic compounds

High melting point
High boiling point
Very strong
Good conductors (Liquid form)

11

Properties of molecular compounds

Low melting point
Low boiling point
Poor conductors
Weaker than ionic

12

How do u know how many atoms are in a compound

CH4 would have 5...
You count the subscripts.. If it's reduced you probably need to unreduce it

13

Types of bonds

Ionic
Covalent(molecular)
Hydrogen
Dipole dipole
London dispersion
Metallic

14

What's VESPR

Has to do with the shape of the molecule like where u do the dot diagrams then figure out the shape .. Tetrahedral, pyramidal, bent, etc

15

What has the highest to lowest boiling point (the types of bonds) AKA what's strongest to weakest bonds

Ionic compound
Hydrogen bonds
Dipole dipole
London dispersion

16

Polar and nonpolar

Polar means it has different charged ends...

Nonpolar means it has the same charged ends

17

How do dipole arrows work

The slightly positive end (lower ELECTRONEGATIVITY) has a plus and then you make an arrow pointing towards the negative side and you make a slightly positive and slightly negative thing on the ends (looks like an unfinished 8) and you put the electronegatitvy difference on top

18

Why are boiling points different between different bonding types

Ionic bonds have the strongest bonds so it takes a lot to break them = highest boiling point
Hydrogen bonds are next strongest bond = next highest boiling point
Dipole dipole are next hardest to break= next highest boiling point
Nonpolar molecules are really easy to break=low boiling point

19

What are covalent bonds

Bonds inside a compound it's the forces found inside of one molecule it's an intramolecular force

20

What's the ELECTRONEGATIVITY for ionic

1.7-3.3

21

What's the electronegativity for polar on that arrow

0.5-1.7

22

What's the electronegativity for nonpolar on that arrow

0-0.5

23

Metals _____ electrons and non metals _____ electrons

Metals give non metals get

24

_______ is positive _______ is negative

Metals are positive nonmetals are negative

25

4-0

Tetrahedral
Got one triangle one dots

26

3-0

Trigonal planar flat

27

3-1

Pyramidal
One triangle one dotted line

28

2-2 / 2-1

Bent
Flat

29

How do the VESPR codes work

The first number is the number of atoms the second is the number of lone pairs on the central atom

30

What's the tie breaker for boiling point

More electrons = higher boiling point

Size of the atom
-small atoms have a higher boiling point

31

How do you know which atoms are bigger and which are smaller

atomic size decreases as you go from the left to the right and it decreases as you go from the bottom to the top

32

London dispersion

All molecules have it... Electrons are always moving so at some points for really quick seconds the molecule can be slightly polar

33

Hydrogen bonding

Polar molecule with hydrogen directly bonded to N, O and F

34

Dipole dipole

Polar molecules... Slightly positive and slightly negative ends