remember when I said that we have to learn some physical properties about transition metals and then I stated that they don't have to follow those normal patterns that we see with the mangle metals and non-metals but they have their own Trends well you'll come to that part of our journey folks we can now kind of get out of periodic table if you like create small trend lines but our Focus for physical properties are going to be um atomic size electro negativity which is going to be affinity for electrons and ionization energy which basically means the energy required to remove an electrons since we are talking about Metal and they tend to be um Ox they tend to form oxidation right or loss of electrons so here you will see transs for our period for um transmiss transmission transition metals here and so I'm just going to write a couple of boundaries just so it's easier for fa things and see those strings so we're going to focus on our atomic radius first and in main group elements atomic size decreases across the period so remember we're going across a period um this is going to be usually from left to right so in our main group elements atomic size is going to decrease across the period but with transition um Metals atomic size decreases at first but then remains relatively constant so we can see there's some increase here with our uh Scandium and titanium but they basically remain constant as we go across the actual period now with electro negativity um when it comes to main groups electro negativity is going to generally increase across the period that's what we usually see for main group elements but as you can see with our transition metals here they have a relatively constant electro negativity okay so as you can see they have kind of a constant here between 1.3 up to 1.9 and then 1.6 and so you can generally say that they have more intermediate electro negativity values again we're only seeing period four so I'm talking in general as well and then finally ionization energy um with main group elements you know ionization energy is going to rise from left to right as we go across but with our transition metals ionization energy is going to be relatively small across the transition metals uh for the period hereo okay so that means that we have relatively small increases so you can see we're still in the 600 still in the 600 yet to to the 700 and now we genuinely stayed there so because we have such small um yes there are increases but the relatively small cross transition metals um this mainly is due to the fact that it's going to be harder to make those electrons kind of have any kind of connection to the nucleus and so what I mean by that is reactivity is all about having that nucleus be able to be attracted to electrons so these bonds can form right but when you have these inner um electrons or de orbital electrons as well sometimes they can Shield the nucleus and because of that you can see it kind of these stable numbers as we go across a period Well if we want across a period what about if we go up and down groups okay well these vertical trains which are going are going to be up and down they also exist as well that means they're also going to be different for our transition metals and they would be for our main group Metals our Focus this time around is going to be still atomic size electron negativity ionization energy but now we're going to include density as well so when we're thinking about atomic size we automatically have to think of volume as well because the larger it is the more space is going to take up and so atomic size and volume are going to be inversely related to density because density is going to equal mass or volume and what this really means is it's just going to tell us how closely packed these atoms are in their solid form so we get to learn more about this in 10.6 chapter of course this could be a small amount of review for Kim 101 as well so let's get to it Atomic side as you can see um for our atomic size or atomic radius the transition metals are going to increase down a group okay so they're going to increase as you go down the group here between four and five but they're basically going to um stop the increase after day so our anytime we're looking at any of these graphs the Orange is going to be our period four the blue or purple is going to be period five and six is also going to be that like lighter blue okay so if we're talking about within a group that means we're going from four up to six here we're going from four up to six four up to six and so that's kind of the trend so when they're saying that we're going down a group for example just think that this is all in Reverse so as we go down this group here um we do see that there is definitely an increase between four and five but then when you get to five and six it's really hard to distinguish these two purple and blue lines here all right electr negativity here there is an increase again between four and five four five and six is going to be this color here so there is increase between four and five but the similar thing is that um it's going to be basically no further increase from between five and six yes there are some exceptions like gold here gold is just very very uh heavy okay so because it's very heavy it actually likes to be more electronegative and can kind of have more of a calent character so there's a lot of smaller details that you can get into when it comes to these transition BS too but a lot of times when you do start seeing um everything kind of merge it's definitely going to be be to uh due to that shielding in those inner electrons shielding that nucleus so that everything kind of remains constant okay now let's go down to ionization energy as you can see really going to generally increase down of groups so again we're going to have our four five and six we kind of see a general increase as you go down a group now if you're going to increase the ionization energy down a group that means you're also going going to have your reactivity decreased okay folks we'll talk about that a little later too and then finally we have our density here so density is going to increase Downer transition group we're definitely going to increase Downer transition group as you can see here um because of those atomic sizes and thus Atomic volume is going to be increased period six or the ones that we see in this white blue here our lanthanides are going to be some of the densest elements not they're not just lanides we know that's our inner transitions they're also going to be like our halfi that we saw earlier as well also examples like gold tungsten Platinum they're all just extremely heavy so we can start recognizing that just based on us understanding electron configuration and atomic properties we now can start building up these physical properties and guess what some things like ionization energy can help us understand reactivity when it comes to chemical properties too and so we'll just continue on to build on to our chemical properties next