Quiz
C4 - Part 1
This quiz has question types that open in the usual player.
Questions in this quiz (28)
1The model of atomic structure has changed over time as...
- Anew evidence has been discovered
- Bnew elements have been discovered
- Cnew developments have been made
2The idea that everything is made from [blank_start]atoms[blank_end] was first put forward in [blank_start]Ancient[blank_end] [blank_start]Greece[blank_end]
- Aatoms
- BAncient
- CGreece
3When [blank_start]John[blank_end] [blank_start]Dalton[blank_end] published his '[blank_start]Atomic[blank_end] Theory' in [blank_start]1803[blank_end] the idea that everything is made from atoms began to gain [blank_start]acceptance[blank_end].
- AJohn
- BDalton
- CAtomic
- D1803
- Eacceptance
4[blank_start]John[blank_end] [blank_start]Dalton[blank_end] imagined atoms to look like [blank_start]billiard[blank_end] balls. His main ideas were:
1.) Elements are made from very tiny [blank_start]particles[blank_end] called [blank_start]atoms[blank_end], which cannot be [blank_start]made[blank_end] or [blank_start]broken[blank_end] up.
2.) [blank_start]Atoms[blank_end] of the same [blank_start]element[blank_end] are [blank_start]identical[blank_end] and [blank_start]different[blank_end] to other elements' atoms.
3.) [blank_start]Atoms[blank_end] combine to make [blank_start]compounds[blank_end].
Now we now that the theory was not [blank_start]100[blank_end]% correct.- AJohn
- BDalton
- Cbilliard
- Dparticles
- Eatoms
- Fmade
- Gbroken
- Helement
- IAtoms
- Jidentical
- Kdifferent
- LAtoms
- Mcompounds
- N100
5[blank_start]J[blank_end].[blank_start]J[blank_end] [blank_start]Thomson[blank_end] discovered that even smaller [blank_start]particles[blank_end] could be pulled out of [blank_start]atoms[blank_end] using a very [blank_start]high[blank_end] [blank_start]voltage[blank_end] ( the discovery of the [blank_start]electron[blank_end]) He pictured the atom to be solid like a [blank_start]currant[blank_end] [blank_start]bun[blank_end] and his experiments [blank_start]removed[blank_end] the [blank_start]currants[blank_end].
A few years later, [blank_start]Ernest[blank_end] [blank_start]Rutherford[blank_end] proved that the atom was not [blank_start]solid[blank_end] but had a very [blank_start]dense[blank_end] [blank_start]centre[blank_end] called a [blank_start]nucleus[blank_end].
[blank_start]Niels[blank_end] [blank_start]Bohr[blank_end] combined his work on the [blank_start]orbits[blank_end] of [blank_start]electrons[blank_end] to develop the idea of the [blank_start]solar[blank_end] system [blank_start]atom[blank_end], the [blank_start]nucleus[blank_end] in the centre like the [blank_start]Sun[blank_end] with the [blank_start]electrons[blank_end] orbiting around it like [blank_start]planets[blank_end]
The ideas at each stage did not fully explain the behaviour of [blank_start]atoms[blank_end]. All the evidence had to be tested and predictions had to be made that would all have to be correct before a new [blank_start]theory[blank_end] was accepted.
Each development was a step closer to understanding the [blank_start]atom[blank_end] and helped other scientists with their work.
Not all experiments went to plan : Rutherford's assistants, [blank_start]Geiger[blank_end] and M[blank_start]arsden[blank_end], expected the [blank_start]alpha[blank_end] particles they were firing at gold [blank_start]foil[blank_end] to punch through in a straight line. A few were [blank_start]deflected[blank_end] and some even [blank_start]bounced[blank_end] straight back leading to the idea that the [blank_start]alpha[blank_end] particles were passing very close to, or hitting, the [blank_start]nucleus[blank_end] of the gold atoms.- AThomson
- BJ
- CJ
- Dvoltage
- Ehigh
- Fparticles
- Gatoms
- Helectron
- Icurrant
- Jbun
- Kremoved
- Lcurrants
- MErnest
- NRutherford
- Osolid
- Pdense
- Qcentre
- Rnucleus
- SNiels
- TBohr
- Uorbits
- Velectrons
- Wsolar
- Xatom
- Ynucleus
- ZSun
- AAelectrons
- ABplanets
- ACatoms
- ADtheory
- AEatom
- AFGeiger
- AGarsden
- AHalpha
- AIfoil
- AJdeflected
- AKbounced
- ALalpha
- AMnucleus
6All substances are made up of very small [blank_start]particles[blank_end] called [blank_start]atoms[blank_end] with a very [blank_start]low[blank_end] [blank_start]mass[blank_end].
Atoms have a [blank_start]central[blank_end] nucleus.
The nucleus is [blank_start]positively[blank_end] charged because it is made up of positive [blank_start]protons[blank_end] and neutral [blank_start]neutrons[blank_end].
The space around the nucleus is occupied by negatively charged [blank_start]electrons[blank_end] arranged in [blank_start]shells[blank_end].
Overall, an atom has [blank_start]no[blank_end] charge.
An atom has the same number of [blank_start]protons[blank_end] and e[blank_start]lectrons[blank_end], so they [blank_start]cancel[blank_end] out each other's charges.- Aparticles
- Batoms
- Clow
- Dmass
- Ecentral
- Fpositively
- Gprotons
- Hneutrons
- Ielectrons
- Jshells
- Kno
- Lprotons
- Mlectrons
- Ncancel
7An element is a substance that cannot be [blank_start]broken[blank_end] down [blank_start]chemically[blank_end] and contains only [blank_start]one[blank_end] type of [blank_start]atom[blank_end].
- Abroken
- Bchemically
- Cone
- Datom
8A compound is a substance that contains at least [blank_start]two[blank_end] elements that are [blank_start]chemically[blank_end] [blank_start]combined[blank_end].
- Atwo
- Bchemically
- Ccombined
9The elements in the Periodic Table are arranged in order of ascending [blank_start]atomic[blank_end] [blank_start]number[blank_end], starting with [blank_start]hydrogen[blank_end] ( atomic number [blank_start]1[blank_end]) at the top.
- Aatomic
- Bnumber
- Chydrogen
- D1
10What is the atomic number?
- AThe number of protons in the atom
- BThe number of neutrons in the atom
- CThe number of protons and neutrons in the nucleus
- DThe number of protons and electrons in the atom
11All atoms of a particular element have the same number of [blank_start]protons[blank_end]. ( Different numbers of [blank_start]protons[blank_end] indicate atoms of different [blank_start]elements[blank_end])
- Aprotons
- Bprotons
- Celements
12Isotopes are varieties of elements with [blank_start]different[blank_end] numbers of [blank_start]neutrons[blank_end]. Isotopes have the same [blank_start]atomic[blank_end] [blank_start]number[blank_end] but a different [blank_start]mass[blank_end] [blank_start]number[blank_end]. The mass number is the [blank_start]total[blank_end] number of p[blank_start]rotons[blank_end] and [blank_start]neutrons[blank_end] in an atom.
- Aneutrons
- Bdifferent
- Catomic
- Dnumber
- Emass
- Fnumber
- Gtotal
- Hrotons
- Ineutrons
13What is the mass number?
- AThe total number of protons and neutrons in an atom
- BThe total number of protons and electrons in an atom
- CThe number of protons in the nucleus
- DThe number of neutrons in the nucleus
14The [blank_start]electrons[blank_end] in an atom occupy the lowest [blank_start]available[blank_end] [blank_start]shell[blank_end]s.
The first [blank_start]energy[blank_end] level or [blank_start]shell[blank_end] can contain a maximum of only [blank_start]two[blank_end] [blank_start]electrons[blank_end].
The [blank_start]outer[blank_end] shell can hold a maximum of [blank_start]eight[blank_end] [blank_start]electrons[blank_end] - an [blank_start]outer[blank_end] shell containing [blank_start]eight[blank_end] electrons is known as a [blank_start]full[blank_end] [blank_start]outer[blank_end] shell.
The electronic structure of an ion can be determined by working out the electronic structure of the atom and [blank_start]adding[blank_end] [blank_start]electrons[blank_end] for a negative ion or [blank_start]subtracting[blank_end] [blank_start]electrons[blank_end] for a positive ion- Aavailable
- Belectrons
- Cenergy
- Dshell
- Etwo
- Felectrons
- Gouter
- Height
- Ielectrons
- Jouter
- Keight
- Lfull
- Mouter
- Nadding
- Oelectrons
- Psubtracting
- Qelectrons
- Rshell
15An uncharged particle is either:
- Aan atom on its own, e.g. Na, Cl
- Ba molecule with two or more atoms bonded together, e.g. Cl2 , C02
- CA charged atom, e.g Na +
- DA group of atoms
16An ion is...
- Aa charged atom of group of atoms, e.g. Na + , Cl -, NH4+ , SO4-
- Ban atom on its own, e.g. Na, Cl
- Ca molecule with two or more atoms bonded together, e.g. Cl2 , or C02
17A positive [blank_start]ion[blank_end] is formed when an [blank_start]atom[blank_end] ( usually a [blank_start]metal[blank_end] ) or group of atoms loses one or more [blank_start]electrons[blank_end].
Losing [blank_start]one[blank_end] electron makes a + ion, e.g. Na+
Losing [blank_start]two[blank_end] electrons makes a 2+ ion, e.g. Mg 2+- Aatom
- Bmetal
- Cion
- Delectrons
- Eone
- Ftwo
18A negative [blank_start]ion[blank_end] is formed when an [blank_start]atom[blank_end] ( usually a [blank_start]non[blank_end] - [blank_start]metal[blank_end] ) or group of atoms [blank_start]gains[blank_end] one or more [blank_start]electrons[blank_end].
Gaining one [blank_start]electron[blank_end] makes a - [blank_start]ion[blank_end], e.g. Cl -
Gaining two [blank_start]electrons[blank_end] make a 2- [blank_start]ion[blank_end], e.g. 02-- Anon
- Bmetal
- Catom
- Dion
- Eelectrons
- Fgains
- Gelectron
- Hion
- Ielectrons
- Jion
19Atoms form [blank_start]ions[blank_end] to gain a [blank_start]full[blank_end] [blank_start]outer[blank_end] [blank_start]shell[blank_end] of [blank_start]electrons[blank_end] as this is a very [blank_start]stable[blank_end] structure.
- Aions
- Bfull
- Couter
- Dshell
- Eelectrons
- Fstable
20A [blank_start]metal[blank_end] and a [blank_start]non[blank_end] [blank_start]metal[blank_end] combine by [blank_start]transferring[blank_end] [blank_start]electrons[blank_end]. The metal atoms transfer [blank_start]electrons[blank_end] to become [blank_start]positive[blank_end] [blank_start]ions[blank_end] and the non - metal atoms [blank_start]receive[blank_end] electrons to become [blank_start]negative[blank_end] [blank_start]ions[blank_end].
The p[blank_start]ositive[blank_end] ions and n[blank_start]egative[blank_end] ions are the [blank_start]attracted[blank_end] to eachother. Two compounds that are [blank_start]bonded[blank_end] by the [blank_start]attraction[blank_end] of oppositely charged ions are s[blank_start]odium[blank_end] c[blank_start]hloride[blank_end] and m[blank_start]agnesium[blank_end] o[blank_start]xide[blank_end].- Ametal
- Bnon
- Cmetal
- Dtransferring
- Eelectrons
- Fpositive
- Gions
- Hreceive
- Inegative
- Jions
- Kelectrons
- Lositive
- Megative
- Nattracted
- Obonded
- Pattraction
- Qodium
- Rhloride
- Sagnesium
- Txide
21Sodium Chloride has a [blank_start]high[blank_end] [blank_start]melting[blank_end] point. It does not conduct [blank_start]electricity[blank_end] when it is [blank_start]solid[blank_end]. However, it can [blank_start]dissolve[blank_end] in [blank_start]water[blank_end], and the solution produced can [blank_start]conduct[blank_end] [blank_start]electricity[blank_end]. It is also able to [blank_start]conduct[blank_end] [blank_start]electricity[blank_end] when it is [blank_start]molten[blank_end].
- Ahigh
- Bmelting
- Celectricity
- Dsolid
- Edissolve
- Fconduct
- Gelectricity
- Hconduct
- Ielectricity
- Jmolten
- Kwater
22Magnesium oxide has a [blank_start]higher[blank_end] melting point than Sodium chloride. It does not [blank_start]conduct[blank_end] [blank_start]electricity[blank_end] when it is [blank_start]solid[blank_end] however is can [blank_start]conduct[blank_end] [blank_start]electricity[blank_end] when it is [blank_start]molten[blank_end]
- Ahigher
- Bconduct
- Celectricity
- Dsolid
- Econduct
- Felectricity
- Gmolten
23Sodium Chloride (NaCl) and Magnesium Oxide (MgO) form [blank_start]giant[blank_end] [blank_start]ionic[blank_end] [blank_start]lattices[blank_end] in which p[blank_start]ositive[blank_end] [blank_start]ions[blank_end] and n[blank_start]egative[blank_end] [blank_start]ions[blank_end] are [blank_start]electrostatically[blank_end] attracted to each other.
Sodium Chloride and Magnesium Oxide have [blank_start]high[blank_end] melting points as the [blank_start]strong[blank_end] [blank_start]attraction[blank_end] between [blank_start]oppositely[blank_end] charged [blank_start]ions[blank_end] has to be overcome for them to [blank_start]melt[blank_end].
The attraction is [blank_start]stronger[blank_end] in Magnesium Oxide than in Sodium Chloride and so Magnesium Oxide has a [blank_start]higher[blank_end] [blank_start]melting[blank_end] point.
They conduct [blank_start]electricity[blank_end] when [blank_start]molten[blank_end] or in [blank_start]solution[blank_end] as the [blank_start]charged[blank_end] [blank_start]ions[blank_end] are free to [blank_start]move[blank_end] about.
When they are [blank_start]solid[blank_end], the [blank_start]ions[blank_end] are held in place and cannot [blank_start]move[blank_end] about, which means they do not [blank_start]conduct[blank_end] [blank_start]electricity[blank_end].- Agiant
- Bionic
- Clattices
- Dositive
- Eions
- Fegative
- Gions
- Helectrostatically
- Ihigh
- Jstrong
- Kattraction
- Loppositely
- Mions
- Nmelt
- Ostronger
- Phigher
- Qmelting
- Rmolten
- Ssolution
- Telectricity
- Ucharged
- Vions
- Wmove
- Xsolid
- Yions
- Zmove
- AAconduct
- ABelectricity
24All ionic compounds are....
- Aneutral substances that have equal chargers on the positive ion(s) and the negative ion(s)
- Bnegatively charged atoms
- Cpositively charged atoms
25When a [blank_start]metal[blank_end] and a [blank_start]non[blank_end] - [blank_start]metal[blank_end] combine, [blank_start]electrons[blank_end] are transferred from one atom to the other to form [blank_start]ions[blank_end]. Each atom then has a complete [blank_start]outer[blank_end] [blank_start]shell[blank_end] ( a [blank_start]stable[blank_end] [blank_start]octet[blank_end]) .
Example: Sodium Chloride
Sodium + Chlorine ------> Sodium Chloride
The sodium atom is in group 1 so it has [blank_start]1[blank_end] electron in its [blank_start]outer[blank_end] shell. The chlorine atom is in group 7 so it has [blank_start]7[blank_end] electrons in its [blank_start]outer[blank_end] shell. The [blank_start]sodium[blank_end] atom transfers the single electron in its [blank_start]outer[blank_end] shell to the [blank_start]chlorine[blank_end] to give both atoms [blank_start]8[blank_end] electrons in their [blank_start]outer[blank_end] shells. The sodium has [blank_start]lost[blank_end] an [blank_start]electron[blank_end] so it becomes [blank_start]positive[blank_end], while the chlorine has [blank_start]gained[blank_end] an [blank_start]electron[blank_end] so it becomes [blank_start]negative[blank_end].- Ametal
- Bnon
- Cmetal
- Delectrons
- Eions
- Fouter
- Gshell
- Hstable
- Ioctet
- J1
- K7
- Louter
- Mouter
- Nouter
- Osodium
- Pchlorine
- Q8
- Router
- Slost
- Telectron
- Upositive
- Velectron
- Wgained
- Xnegative
26On the periodic table, the vertical coloums/ [blank_start]groups[blank_end] indicate how many [blank_start]electrons[blank_end] in the [blank_start]outer[blank_end] [blank_start]shell[blank_end]. The horizontal rows / [blank_start]periods[blank_end] indicate how many [blank_start]shells[blank_end] the atom has.
- Agroups
- Belectrons
- Couter
- Dshell
- Eperiods
- Fshells
27The elements on the periodic table are arranged in order of [blank_start]ascending[blank_end] [blank_start]atomic[blank_end] [blank_start]number[blank_end], and then arranged in [blank_start]periods[blank_end] (rows) so that elements with similar [blank_start]properties[blank_end] are in the same [blank_start]group[blank_end] ( column) .
- Aascending
- Batomic
- Cnumber
- Dperiods
- Eproperties
- Fgroup
28More than .... of the elements on the periodic table are metals. The others are non metals.
- A3/4
- B1/4
- C2/3
- D1/2
Information
- Description
- GCSE Chemistry Quiz on C4 - Part 1, created by Verity Cartwright on 15/03/2017.
- Author
- Verity Cartwright
- Language
- English
- Views
- 5
- Tags
- Rating
- No ratings yet Rate this quiz