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Chem > Atomic Structure and Bonding unit > Flashcards

Atomic Structure and Bonding unit Flashcards

1
Q

Octet rule

A

tendancy of atoms to prefer to have 8 electrons in the valence shell

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2
Q

Valence shell electrons

A

electrons which are lost or gained to form ions

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3
Q

Vertical columns on periodic table

A

Groups

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4
Q

Horizontal columns on periodic table

A

Periods

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5
Q

Elements in group 7 are called

A

halogens

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6
Q

Elements in group 8 have _____ ___________ ______ and are called _________

A

full valence shell; noble gases

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7
Q

Charge of nucleus

A

positve

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8
Q

How is a sulfide ion formed? Draw

A
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9
Q

Describe ionic compounds

A

ionic compounds are formed during a reaction between a metal atom and a non-metal atom. The metal atom loses electrons forming positively charged ions called cations, and the non-metal atom gains electrons foorming negative ions called anions. The ions are held together by the electrostatic force of attraction of the oppositely charged atoms.

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10
Q

What is an ionic bond

A

electrostatic force of attraction between oppositely charged ions.

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11
Q

Lattice

A

regular repeated 3D arrangement

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12
Q

Giant

A

unlimited amount of ions, cant state how many ions there are

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13
Q

SO4^2-

A

sulfate

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14
Q

Hydroxide

A

OH-

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15
Q

Carbonate

A

CO3^2-

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16
Q

Nitrate

A

NO3^-

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17
Q

Phosphate

A

PO4^3-

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18
Q

Hydrogen Carbonate

A

HCO3^-

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19
Q

Ammonium

A

NH4^+

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20
Q

Cyanide

A

CN^-

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21
Q

Polyatomic meaning

A

composed of two or more atoms covalently bonded

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22
Q

describe what happens when lithium chloride forms in terms of e- transfer (5)

A

-lithium loses one electron
chlorine gains one e-
lithium has pos charge (cation)
chlorine has neg charge (anion)
electrostatic force of attraction b/w opposite charge

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23
Q

Non- metal and metal bonding

A

Ionic

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24
Q

Why do ionic compunds have high melting and boiliing points

A

It is a giant ionic structure and the strong electrostatic force of attraction between ions require a lot of heat energy to break

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25
Q

Why are ionic compounds soluble in water

A

Water molecules are able to break the electrostatic force of attracytion between ions because water is polar
page 47

26
Q

Why dont ionic solids conduct electricity

A

Fixed structure and ions arent free to move or carry charge

27
Q

Why do ionic liquids conduct electricity

A

Ions can move past eachother and charge can flow, making a electric current.

28
Q

Brittle meaning

A

When a force is applied, ions in lattice shift so that like ions repel and lattice breaks

29
Q

Hard

A

strong electrostatic force of atraction between oppositely charged ions

30
Q

AMMONIUM TEST

A

add dilute sodium hydroxide (NaOH) solution
gently heat
if NH4 present, pungent smell, identified using damp red litmus paper held above test tube

31
Q

CARBONATE TEST

A

add dilute hydrochloric acid
bubble gas through limewater
if present, limewater turns cloudy

32
Q

SULFATE TEST

A

add dilute hydrochloric acid
add drops of barium chloride
if present, white precipitate forms

33
Q

Halide ions egs

A

cl
br
I

34
Q

HALIDE ION TEST

A

add dilute nitric acid
add drops of silver nitrate solution
if Cl, white precipitate
if Br, cream precipitate
if I, a yellow precipitate

35
Q

Test used for lithium, Sodium, Pottasium or Calcium

A

Flame test

36
Q

FLAME TEST

A

Red= lithium
yellow/orange = sodium
Purple= Pottassium
Brick red= calcium

37
Q

precipitate

A

an insoluble solid formed from two soluble solutions

38
Q

general properties of metals

A

high M = B points
good conductors of heat/ electricity
hard
malleable
ductile

39
Q

which electrons become dlve-

A

valence shell e-

40
Q

Metallic Bonding

A

Lattice of Metal cations are atracted to the sea of dlve-. This electrostatic force of attraction is called metallic bonding.

41
Q

what name is given to structure that simple covalent compounds form

A

Molecule

42
Q

Simple covalent bond characteristics

A

Low M + B points
Not electrically conductive
exhibit weak intermolecular forces.
Not soluble in water

43
Q

Giant covalent bond characteristics

A

High M+B Points
Not electrically conductive
exhibit strong covalent bonding
Not soluble in water

44
Q

Why metals conduct electricity

A

dlve- can move through the structure and carry charge

45
Q

Why metals conduct heat

A

dlve- can move fastly and pass energy on quickly. The lattice of electrons transmits energy efficiently, as atoms vibrate and bump into other atoms

46
Q

Why metals have high M+B points

A

Electrostatic forces of attraction between dlve- and cations are strong and require a lot of heat energy to break them

47
Q

wHY metals malleable

A

arrangement of atoms change but the attraction between dlve- and cations isnt broken

48
Q

Metallic bond characteristic

A

high M+ B points
electrically conductive
Hard and malleable
Not soluble in water

49
Q

Alloy

A

Combinations of two or more metals

50
Q

Alloy characteristics

A

harder than pure metals
less malleable than pure metals
poorer conductors than pure metals

51
Q

Covalent bonding

A

electrostatic force of attraction between the nuclei of two atoms and shared pair of electrons between them

52
Q

Covalent bonnd x2

A

Chemical bond that involves the sharing of valence electron pairs between atoms, forming between non-metal elements. Very strong bonds.

53
Q

structural formula of HCN

A

H-C—N

54
Q

What does it mean to say ionic compunds are mostly soluble in water

A

Water is polar

55
Q

Polarity

A

Nucleus has pull on electrons
strength of pull depends on atom
produces slight charge

56
Q

Is CH4 polar or non polar

A

Non polar

57
Q

Giant covalent structures

A

Many atoms joined to adjacent atoms by covalent bonds
Arranged into giant ionic lattices extremely strong structures because of many bonds.

58
Q

simple covalent molecules consist of a small number of atoms bonded together through___________ _______.

A

simple covalent molecules consist of a small number of atoms bonded together through covalent bonds

59
Q

Allotrope, with example

A

dif forms of same element in same state
eg graphite, diamond

60
Q

Giant cov substances having high M+B points

A

a lot of simple covalent bonds requiring high temps to M/B

Chem (1 decks)

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