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Chemistry > Unit 4 > Flashcards

Unit 4 Flashcards

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1
Q

Ion

A

Charged particle (+/-)

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2
Q

1 atom

A

Monatomic ion

Ex. Na+

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3
Q

2+ atoms

A

Poly atomic ion

PO 4-

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4
Q

Cation

A

Positive ion

Formed from a loss of electrons

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5
Q

Anion

A

Negative ion

Formed from a gain of electrons

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6
Q

What do cations form from?

What do anions form from?

A

Metals

Nonmetals

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7
Q

Naming cations & anions

A

Keep the name of atom and add ion

Change end of atom name to ide and add io

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8
Q

Chemical bond

Why do bonds form?

A

An attentive force between atoms and ions that binds them together as a unit
Form to:
-decrease potential energy
-increase stability

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9
Q

Compound

A

A pure substance made of 2 or more elements chemically combined together

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10
Q

Molecule

A

Compounds that are made by the sharing of electrons

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11
Q

Binary compound

Ternary compound

A

Binary-2 different elements ex. CaF2

Ternary-3 or more different elements ex. NaNO3

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12
Q

Ionic bonds

A

A bond formed from the transfer of electrons (one atom loses an electron and the other gains them)
Often referred to as salts

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13
Q

What types of atoms can form ionic bonds?

A
  • metals and non metals
  • metals and poly atomic ions
  • ploy atomic ions and Nonmetals
  • 2 poly atomic ions
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14
Q

Structure of ionic bonds

A

Crystal lattice structure-positive and negative ions stack up so they can be near an ion of opposite charge

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15
Q

Strength of ionic bonds

A

Very strong

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16
Q

Melting/boiling points of ionic bonds

A

Very high melting and boiling points because the bonds are very strong and require lots of energy to break them

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17
Q

Conductivity of ionic bonds

Do they conduct through solids?

A

Can only conduct electricity when dissolved in water or molten (melted)
Do not conduct through solids

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18
Q

Covalent bonds

A

Formed when 2 atoms share electrons in order to satisfy the octet rule
There are no cations or anions because they are sharing electrons (no charge)

19
Q

What types of atoms can covalent bonds form?

A

Formed from Nonmetals only

20
Q

What is the structure of covalent bonds?

A

Structure can vary

21
Q

Strength of covalent bonds

A

Very weak compared to ionic bonds because there is no charge holding them together

22
Q

Melting and boiling points of covalent bonds

A

Low melting and boiling points because they are a weak type of bond and requires low energy to break them

23
Q

Conductivity of covalent bonds

A

Do not conduct electricity in water because they do not break apart into ions like ionic compounds so electrons can’t flow through

24
Q

Polar covalent bonds

A

Atoms are NOT equally sharing electrons because one of the electrons is stronger
Partial charge due to unequal sharing

25
Q

Nonpolar covalent bonds

A

Atoms are equally sharing electrons

No charge due to equal sharing

26
Q

Polarity is the difference in _________ of the atoms bonded together

A

Electromagnetivity-the ability of an atom to pull electrons towards itself

27
Q

Bond length

A

NP covalent > Polar covalent > ionic

28
Q

Bond strength

A

Ionic > Polar covalent > NP covalent

29
Q

Electromagnitivity for NPC, PC, and ionic

A

NPC-less than 0.5
Difference is greater than 1.7-ionic
Difference is greater than 0.5-polar covalent

30
Q

Atom

A

Smallest particle that makes all things

Neutral

31
Q

MX

A

Linear

32
Q

MX2

A

Linear

33
Q

MX3

A

Trigonal planar

34
Q

MX4

A

Tetrahedral

35
Q

MX2E

A

Bent

36
Q

MX2E2

A

Bent

37
Q

MX3E

A

Trigonal pyramid

38
Q

VSEPR (Valence Shell Electron Pair Repulsion) Theory

A

Electrons carry a negative charge and will repel other electrons due to like charges. Due to this electrons (lone pair and bonds) will spread out as far as possible thus creating a certain molecular shape around the central atom

39
Q

What are shapes determined by?

A

The repulsive forces between shared and unshared electron pairs

40
Q

When writing a formula for ionic compounds, which ion goes first?

A

The cation goes first and the anion goes second

41
Q

Rules for naming a binary ionic compound

A

The metal (the cation) keeps its name, but the anion keeps the root of the name and gets the ending changed to -ide

42
Q

Rules for naming transition metals

A

Keeps the element name, but charge is written in Roman Numerals

43
Q

Which transition metals do not have variable charges?

A

Zinc: Zn2+
Silver: Ag+
Cadmium: Cd2+

44
Q

Naming covalent molecules

A

Determine the prefix for each nonmetal

Chemistry (11 decks)

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