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Science > Chem Unit 5 > Flashcards

Chem Unit 5 Flashcards

1
Q

Ions

A

Atoms that lose or gain electrons

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2
Q

The Ocet Rule

A

Atoms will gain or lose atoms in order to completely fill up the outermost shell with 8 electrons

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3
Q

Ionic bond basic

A

At least one metal and one nonmetal, electrons are transferred from metal to nonmetal

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4
Q

Covalent bond basic

A

Only non metals, electrons are shared between no metals

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5
Q

Metallic bond basic

A

Only metals, electrons are delocalized

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6
Q

Type of structure of bonds

A

Ionic- crystal lattice
Covalent- true molecules
Metallic- “electron sea” or crystal structure

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7
Q

Phase at room temp and melting point

A

Ionic- solid at room temp, high melting point
Covalent- liquid or gas at room temp, low melting point
Metallic- solid at room temp, very high melting point

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8
Q

Solubility and electrical conductive kitty

A

Ionic- soluble, conducts electricity but only when dissolved in water or in liquid form
Covalent- usually not double, not a conductor
Metallic- not soluble, conducts electricity

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9
Q

Covalent bond

A

An electrostatic attraction of electrons to two different nuclei that holds the nuclei together

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10
Q

Purpose of bonds between atoms

A

To increase stability of the neutral atom

To decrease potential energy (the bond energy)

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11
Q

Naming monatomic ion

A

for a cation leave the name as is
For anions drop the end and add -
ide

(Oxide)

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12
Q

Naming binary ionic compounds

A

Metal/Cation goes first, nonmetal/anion goes last
When determining formula from compound name, add enough molecules so positive charge equals negative charge
NaCl)

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13
Q

Naming transition metals

A

Charge of ion must be indicated in name of compound

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14
Q

Polyatomic ions

A

Ions made up of covalent my bonded atoms that have an overall charge, with special names

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15
Q

Ammonium

A

NH4+1

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16
Q

Hydroxide

A

OH-1

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17
Q

Carbonate

A

CO3-2

18
Q

Chlorate

A

ClO3-1

19
Q

Chlorite

A

ClO2-1

20
Q

Cyanide

A

CN-1

21
Q

Nitrate

A

NO3-1

22
Q

Nitrite

A

NO2-1

23
Q

Phosphate

A

PO4-3

24
Q

Phosphite

A

PO3-3

25
Q

Sulfate

A

SO4-2

26
Q

Sulfite

A

SO3-2

27
Q

Naming covalent compounds

A

Prefixes identify number of each element in the name

28
Q

Prefixes

A 
1-mono
2-di
3-tri
4-tetra
5-penta
6-hexa
7-hepta
8-octa
9-nona
10-deca
29
Q

Saturated vs unsaturated hydrocarbons

A

Saturated is the there is the maximum number of hydrogen atoms connected to the available carbons, and unsaturated means there’s at least one double or triple bond

30
Q

Alkanes

A

A hydrocarbon where there are only single covalent bonds between the carbon and hydrogen atoms

31
Q

Alkenes

A

At least one double bond in the carbon-carbon bond

32
Q

Alkynes

A

At least one or more triple covalent bond

33
Q

Structures vs condensed formula

A

Structured shows position of every single atom, while condensed shows the bonds in groupings (CH3-CH2-CH3)

34
Q

Line Angle Formula

A

Carbons and hydrogen atoms are removed. Bonds between carbons shown as a “zigzag” line, but all other atoms are shown

35
Q

Prefixes for naming Alkanes

A 
1-meth
2-eth
3-prop
4-but
5-pent
6-hex
7-hept
8-oct
9-non
10-dec
36
Q

Structural isomers

A

Molecules that have the same molecular formulas but a different arrangement of atoms (different structural formulas)

37
Q

Geometric isomers

A

Have atoms joined in the same order, but differ in the orientation of groups around a double bond

38
Q

Cis configuration

A

The substituent groups are on the same side of the double bond

39
Q

Trans configuration

A

The substituent groups are on opposite sides of the double bond

40
Q

Lewis dot diagram

A

Write element symbol, then draw in number of valence electrons around it

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